Free Printable Chemistry Final Exam Review Units 7-9

1.

The following is what type of reaction:
PbCl₂ + AgNO₃ → Pb(NO₃)₂ + AgCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

2.

The following is what type of reaction:
NH₃ + HCl → NH₄Cl

a)

Synthesis

b)

Decomposition

c)

Single Replacement Replacement

d)

Double Replacement Replacement

3.

What type of chemical reaction is this?
Al(OH)₃ → Al₂O₃ + H₂O

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

4.

Ions in two compounds switch.

a)

Synthesis

b)

Combustion

c)

Single Replacement

d)

Double Replacement

5.

3Ca + 2AlCl₃ --> 3CaCl₂+2Al

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

6.

One reactant into several products.

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

7.

Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water.

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

8.

Two Reactants and One Product

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

9.

4Si + S₈ --> 2Si₂S₄

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

10.

C₄H₁₂ + O₂ → CO₂ + H₂O

a)

Synthesis

b)

Combustion

c)

Single Replacement

d)

Double Replacement

11.

2Pb(NO₃)₂ --> 2PbO + 4NO₂ + O₂

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Combustion

12.

3Mg + N₂ --> Mg₃N₂

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Combustion

13.

2NO₂ --> N₂+ 2O₂

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Combustion

14.

P₄ + 3O₂--> 2P₂O₃

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Combustion

15.

4Si + S₈ --> 2Si₂S₄

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

16.

3KOH + H₃PO₄ --> K₃PO₄+3H₂O

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Double displacement

17.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

18.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

19.

What reaction has the following general formula:

AB + CD --> CB + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

20.

What reaction has the following general formula:

A + B --> AB

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

21.

Based on the information provided, which type of reaction is this?

RS ➔ R + __________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

22.

What is the missing product?

RS ➔ R + __________

a)

RS

b)

S

c)

T

23.

Based on the information provided, what type of reaction is this?

RS + TU ➔ RU + _________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Combustion

24.

What is the missing product?

RS + TU ➔ RU + _________

a)

S

b)

T

c)

TS

25.

Based on the information provided, what type reaction is this?

C_xH_y + O₂ ➔ CO₂ + __________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Combustion

26.

What is the missing product?

C_xH_y + O₂ ➔ CO₂ + __________

a)

H₂O

b)

HO

c)

CHO

27.

Based on the information provided, what type of reaction is this?

R + ST ➔ RT + _________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

28.

What is the missing product?

R + ST ➔ RT + _________

a)

R

b)

T

c)

S

29.

Based on the information provided, which type of reaction is this?

R + S ➔ _________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

30.

What is the missing product?

R + S ➔ _________

a)

R

b)

S

c)

RS

31.

Based on the information provided what type of reaction it this?

Au₂S₃ + 3 H₂ ➔ 2 Au + ____________

a)

Combustion

b)

Single replacement

c)

Double replacement

d)

Synthesis

32.

What would the missing product be?

Au₂S₃ + 3 H₂ ➔ 2 Au + ____________

a)

2 H₃S

b)

2 AuH₃

c)

3 H₂S

33.

Based on the information provided, what type of reaction is this?

CH₄ + 2 O₂ ➔ CO₂ + ___________

a)

Double replacement

b)

Single Replacement

c)

Decomposition

d)

Combustion

34.

What would the missing product be?

CH₄ + 2 O₂ ➔ CO₂ + ___________

a)

2 H₂O

b)

4 HO

c)

CO₂

35.

Based on the information provided, what type of reaction is this?

Fe + O₂ ➔ ___________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

36.

What would the missing product be?

Fe + O₂ ➔ ___________

a)

Fe₂O₂

b)

2 FeO

c)

2 FeOH

37.

Based on the information provided, what type of reaction is this?

Na₂CO₃ + 2 AgNO₃ ➔ 2 NaNO₃ + __________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

38.

What is the missing product?

Na₂CO₃ + 2 AgNO₃ ➔ 2 NaNO₃ + __________

a)

2 Ag₃Na

b)

2 AgCO₃

c)

Ag₂CO₃

39.

Based on the information provided, what type of reaction is this?

2 NO₂ ➔ O₂ + _________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

40.

What is the missing product?

2 NO₂ ➔ O₂ + _________

a)

N₂

b)

N

c)

NO

41.

A list of elements that organizes them in order of their reactivity is called

a)

Negativity Series

b)

Netflix Series

c)

Activity Series

d)

Displacement Series

42.

Which one of the following would result in a displacement reaction?

a)

Iron with magnesium chloride

b)

magnesium with iron chloride

c)

Iron with Zinc Sulphate

d)

gold with silver nitrate

43.

A displacement reaction will occur when...

a)

a more reactive metal displaces a less reactive metal from its compound.

b)

A less reactive metal displaces a more reactive metal from its compound

c)

Displacement only occurs when two of the same metals are reacted

d)

Displacement reactions will only occur in metals above iron in the reactivity series

44.

Which metal is more reactive than calcium?

a)

magnesium

b)

potassium

c)

silver

d)

aluminum

45.

Which of the following metals is the most reactive according to the reactivity series of metals.

a)

Copper

b)

Zinc

c)

Magnesium

d)

Lithium

46.

Based on the activity series, which metal could X represent in the reaction below?

X + Calcium nitrate —> Calcium + X nitrate

a)

Ba

b)

Fe

c)

Mg

d)

Zn

47.

Which of the following will not undergo reaction?

a)

zinc metal + zinc oxide

b)

iron metal + copper oxide

c)

zinc metal + iron oxide

d)

magnesium + iron oxide

48.

The following reaction occurs. It shows that

X + ZY --> ZX + Y

a)

Z replaced X

b)

Y is more reactive than X

c)

X is more reactive than Y.

d)

Y has changed into a new compound.

49.

What will be the result if a less reactive metal is added in a solution with more reactive metal compound?

a)

vigorous reaction

b)

fizzing gas produced

c)

burns moderately

d)

no reaction

50.

When a metal reacts with oxygen gas, the product is ...

a)

metal hydroxide

b)

metal oxide

c)

metal oxide and oxygen

d)

metal hydroxide and hydrogen gas

51.

Which is not a Alkali Metal?

a)

Lithium

b)

Sodium

c)

Gold

d)

Potassium

52.

When scrap iron is added to blue copper sulphate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pale green solution is of?

a)

iron oxide

b)

copper chloride

c)

sulphuric acid

d)

iron sulphate

53.

Will silver react with magnesium chloride solution?

a)

yes

b)

no

54.

Determine the result of the following potential reaction.

Nickel added to cold water .

a)

Nickel added to cold water produces nickel hydroxide and hydrogen gas.

b)

Nickel added to cold water produces nickel oxide and hydrogen gas.

c)

No Reaction

55.

Which compound is higher in reactivity, Ag or Ca?

a)

Ag

b)

Ca

c)

Neither

d)

They're equal

56.

Indicate which of the following is more reactive.

a)

FLUORINE

b)

BROMINE

57.

Indicate which of the following is more reactive.

a)

Tin

b)

Barium

58.

Which of the following metals is the most reactive according to the reactivity series of metals.

a)

Copper

b)

Zinc

c)

Magnesium

d)

Lithium

59.

Indicate which of the following is more reactive.

a)

Iron

b)

Magnesium

60.

Determine the result of the following potential reaction.

Potassium added to cold water .

a)

Potassium added to cold water produces potassium hydroxide and hydrogen gas.

b)

Potassium added to cold water produces potassium oxide and hydrogen gas.

c)

No Reaction

61.

A mixture contains cobalt metal, copper metal, and tin metal. This mixture is mixed with nickel nitrate. Which metals, if any, will react?

a)

Cobalt only

b)

Copper only

c)

Tin only

d)

All 3

62.

Identify ALL evidences of a chemical reaction.

a)

Change of state (liquid to gas)

b)

Color change

c)

Temperature change

d)

Tearing a paper

e)

Burning a paper

63.

Which statement below describes a PHYSICAL change?

a)

Burning the crust of the bread when making toast.

b)

Placing waffles in the toaster and applying butter on it.

c)

Frying an egg to make an egg sandwich.

d)

Using a cookie cutter to make heart-shaped cookies.

64.

When a chemical change occurs, ____________ with ___________ is formed.

a)

a new substance

b)

different properties

c)

the same substance

d)

same properties

65.

Which of the following examples shows that a chemical reaction has occurred?

a)

A rock breaks into smaller pieces when it is struck with a hammer.

b)

Rust forms on a hammer that has been left outside to long.

c)

A cup of water turns pink when a few drops of red food coloring are added.

d)

A solid is formed when heat is removed from a sample of water.

66.

A student places a piece of a potato into a container of hydrogen peroxide. One observation the student makes is that bubbles form around the potato. The presence of bubbles might indicate the formation of a new substance because bubbles -

a)

could show that a gas is forming

b)

always rise to the top of a liquid.

c)

are almost always perfectly spherical.

d)

usually burst after a few minutes.

67.

Hydrogen peroxide breaks down to form water and oxygen gas. Which observation is evidence that a chemical reaction has occurred?

a)

The mass of the solution remains the same.

b)

Phase changes are observed.

c)

The color of the solution remains clear.

d)

The temperature of the solution increases.

68.

A clear liquid from a flask is poured into another clear liquid in a beaker. Which of the following results of this procedure would indicate a new substance was formed?

a)

The level of the substance in the beaker is higher after the other liquid is added.

b)

A yellow solid forms and then settles to the bottom of the beaker.

c)

Small white crystals are left behind in the flask that held the first liquid.

69.

Which of the following is an example that includes evidence of a chemical reaction?

a)

A sample of zinc is placed in water and it settles to the bottom

b)

A solid block of ice is heated and it completely melts into a liquid.

c)

Sugar that is burned gives off an odor and turns brown and then black.

d)

A tomato is placed into a blender and chopped up into smaller pieces.

70.

A precipitate is a

a)

liquid that forms when two solids are reacted

b)

a solid that forms when two liquids are mixed

c)

a gas that forms when vinegar and baking soda react

d)

a change of color in a solution

71.

If reaction starts with 20g of reactants it should produce

a)

a total of 40g of products

b)

a total of 10g of products

c)

a total of 80 g of products

d)

a total of 20g of products

72.

What is the Law of Conservation of mass?

a)

Mass is created in a chemical reaction

b)

Mass is created in a physical change

c)

New chemicals formed from a chemical reaction have a larger overall mass than the original reactants

d)

Mass is never created or destroyed

73.

One of the signs of a chemical reaction taking place is:

a)

Bubbles are produced

b)

Reactants are not combining

c)

Products are not forming

d)

Color is not changing

74.

Which is NOT an indication of a chemical change?

a)

temperature change

b)

formation of a precipitate

c)

shape change

d)

production of light

75.

You know you a chemical reaction has occurred if

a)

there is a precipitate.

b)

there is a color change.

c)

there is a temperature change.

d)

All of these answers are evidence.

76.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of HgO to Hg

a)

2:2

b)

1:1

c)

2:1

d)

1:2

77.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of HgO to $O_2$

a)

2:2

b)

1:1

c)

2:1

d)

1:2

78.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of Hg to $O_2$

a)

2:2

b)

1:1

c)

2:1

d)

1:2

79.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $NH_3$ to $NO$

a)

4:5

b)

1:1

c)

2:3

d)

4:6

80.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $NH_3$ to $N_2$

a)

4:5

b)

1:1

c)

2:3

d)

5:6

81.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $N0$ to $N_2$

a)

4:5

b)

1:1

c)

6:5

d)

5:6

82.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $H_2O$ to $N_2$

a)

4:5

b)

1:1

c)

6:5

d)

5:6

83.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $H_2O$ to $LiOH$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

84.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $H_2O$ to $CO_2$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

85.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $CO_2$ to $Li_2CO_3$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

86.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation....
If I decompose 34 moles of HgO, how many moles of oxygen will I produce? What will the ratio that you use look like in this problem?

$\frac{34\ moles\ HgO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{1mole\ O_2}{2\ mole\ HgO}$

b)

$\frac{2\ mole\ HgO}{1\ mole\ O_2}$

c)

$\frac{2\ mole\ Hg}{1\ mole\ O_2}$

87.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation.... $4NH_3+6NO\rightarrow5N_2+6H_2O$
Bacteria will cause ammonia $NH_3$ to react with NO to put nitrogen back in the air, along with water, as part of the nitrogen cycle. If there are 3.56 moles of NO in the soil, how many moles of ammonia are needed to react with it?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{4\ mole\ NH_3}$

b)

$\frac{2\ mole\ NH_3}{3\ mole\ NO}$

c)

$\frac{6\ mole\ Hg}{5\ mole\ N_2}$

88.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation.... $4NH_3+6NO\rightarrow5N_2+6H_2O$
How many moles of water will be produced with 3.56 moles of NO in the soil?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{6\ mole\ H_2O}$

b)

$\frac{1\ mole\ H_2O}{1\ mole\ NO}$

c)

$\frac{6\ mole\ H_2O}{5\ mole\ N_2}$

89.

2Al + 3H₂SO₄ -> Al₂(SO₄)₃ + 3H₂
How many grams of aluminum sulfate would be formed if 250g H₂SO₄ completely reacted with aluminum?

a)

0.85 g

b)

290 g

c)

450 g

d)

870 g

90.

How many grams are in 7.8 moles of NaCl?

a)

476 grams

b)

460 grams

c)

452 grams

d)

462 grams

91.

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from 6 moles H₂?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

92.

One mole of sulfur (S) is equal to home many atoms?

a)

32 atoms

b)

16 atoms

c)

1.20 x 10²³ atoms

d)

6.022 x 10²³ atoms

93.

B₂H₆ + 3O₂ -->2 HBO₂ + 2 H₂O
What mass of O₂ will be needed to burn 36.1 g of B₂H₆?

a)

13.8 g O₂

b)

3.86 mol of O₂

c)

124 g O₂

94.

For the Balanced Reaction:
3 Mg + 1 Fe₂O₃ → 3 MgO + 2 Fe;
What is the Ratio of moles of Mg to moles Fe?

a)

3mol Mg / 2 mol Fe

b)

2 mol Mg/ 3 mol Fe

c)

1 mol Fe/ 2 mol Fe

d)

3 mol MgO / 2 mol Fe

95.

1 N₂ + 3 H₂ --> 2 NH₃

How many moles of NH₃ will be produced from 10.2 x 10^25 molecules of H₂?

(6.02 x 10^23 molecules H₂= 1 mol H₂)

a)

113 mol NH₃

b)

254 mol NH₃

c)

169 mol NH₃

d)

508 mol NH₃

96.

Given the equation:

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

When 2.00 moles of NaClO₃ react, how many grams of O₂is produced?

a)

56 g of O₂

b)

96 g of O₂

c)

64 g O₂

d)

32 g O₂

97.

2 NaClO₃ (s) → 2NaCl (s) +3 O₂ (g)

How many grams of O₂will be produced from 12.00 moles of NaClO₃?

a)

256 g of O₂

b)

576 g of O₂

c)

288 g O₂

d)

32 g O₂

98.

CH₄ + 2 O₂ → CO₂ + 2 H₂O

How many moles of carbon dioxide are produced from the combustion of 110 g of CH₄?

a)

13.7 mol

b)

2.75 mol

c)

6.11 mol

d)

6.85 mol

99.

What is a limiting reactant?

a)

the reactant that determines how much product can be made

b)

the reactant that is in excess

c)

the product that you can make the most of

d)

the amount of reactants that react with each other

100.

You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich. If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?

a)

bread

b)

jelly

c)

peanut butter

d)

sandwich

101.

When 12 moles of O₂ reacts with 1.1 mole of C₁₀H₈what is the limiting reactant? C₁₀H₈ + 12 O₂ --> 10 CO₂ + 4 H₂O

a)

Oxygen

b)

C₁₀H₈

c)

Water

d)

Carbon Dioxide

102.

Use the equation 2 Al + 3 Cl₂ ---> 2 AlCl₃. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl3

b)

Cl2

c)

Al

103.

CH₄ + 2H₂O --> CO₂+ 4H₂What is the limiting reactant when 20g CH₄react with 15g H₂O?

a)

CH₄

b)

H₂O

c)

CO₂

d)

H₂

104.

Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?

a)

Fe

b)

S

c)

FeS

d)

none

105.

SO₂+ PCl₅--> SOCl₂+ POCl₃
How much SOCl₂is produced when 16.2g SO₂react with 13.7g PCl_5?

a)

7.87g

b)

30.1g

c)

26.4g

d)

19.8g

106.

The limiting reactant

a)

slows the reaction down

b)

is used up first

c)

is the reactant that is left over

d)

controls the speed of the reaction

107.

Use the equation 2 Al + 3 Cl₂ ---> 2 AlCl₃. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl₃

b)

Cl₂

c)

Al

108.

When does a chemical reaction stop?

a)

When the lab is finished

b)

When the excess reactant is used up

c)

When the limiting reactant is used up

d)

Chemical reactions never stop

109.

What is the limiting reactant if 10 moles of NH₃ react with 30.0 moles of NO?
4NH₃+6NO --> 5N₂ + 6H₂O

a)

NH₃

b)

NO

c)

N₂

d)

water

110.

P₄+ 3O₂--> P₄O₆
What is the limiting reactant is 12 moles of P₄react with 15 moles of O₂?

a)

P₄

b)

O₂

c)

P₄O₆

d)

none of the above

111.

4NH₃+ 5O₂--> 4NO + 6H₂O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen?

a)

0.37g

b)

0.045g

c)

1.35g

d)

11.1g

112.

Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?

a)

Fe

b)

S

c)

FeS

d)

none

113.

2 NaCl + Pb(NO₃)₂ --> 2 NaNO₃ + PbCl₂

How many grams of lead II chloride are produced from the reaction of 15.3 g of NaCl and 60.8 g of Pb(NO₃)₂?

a)

21.5g

b)

51.1g

c)

43.4g

d)

36.4g

114.

2Al + 3H₂SO₄ -> Al₂(SO₄)₃ + 3H₂
How many grams of aluminum sulfate would be formed if 250g H₂SO₄ completely reacted with aluminum?

a)

0.85 g

b)

290 g

c)

450 g

d)

870 g

115.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of HgO to Hg

a)

2:2

b)

1:1

c)

2:1

d)

1:2

116.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of HgO to $O_2$

a)

2:2

b)

1:1

c)

2:1

d)

1:2

117.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$2HgO\ \rightarrow\ 2Hg\ +\ O_2$
What is the ratio of Hg to $O_2$

a)

2:2

b)

1:1

c)

2:1

d)

1:2

118.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $NH_3$ to $NO$

a)

4:5

b)

1:1

c)

2:3

d)

4:6

119.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $NH_3$ to $N_2$

a)

4:5

b)

1:1

c)

2:3

d)

5:6

120.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $N0$ to $N_2$

a)

4:5

b)

1:1

c)

6:5

d)

5:6

121.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following BALANCED chemical equation to determine the ratio:
$4NH_3+6NO\ \rightarrow\ 5N_2+6H_2O$
What is the ratio of $H_2O$ to $N_2$

a)

4:5

b)

1:1

c)

6:5

d)

5:6

122.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $H_2O$ to $LiOH$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

123.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $H_2O$ to $CO_2$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

124.

BALANCED chemical equations tell you the relative amounts or the ratios of reactants and products.

Use the following UNBALANCED chemical equation to determine the ratio:
$CO_2\ +\ LiOH\ \rightarrow\ Li_2CO_3\ +\ H_2O$
What is the ratio of $CO_2$ to $Li_2CO_3$

a)

1:1

b)

1:2

c)

2:2

d)

2:1

125.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation....
If I decompose 34 moles of HgO, how many moles of oxygen will I produce? What will the ratio that you use look like in this problem?

$\frac{34\ moles\ HgO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{1mole\ O_2}{2\ mole\ HgO}$

b)

$\frac{2\ mole\ HgO}{1\ mole\ O_2}$

c)

$\frac{2\ mole\ Hg}{1\ mole\ O_2}$

126.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation.... $4NH_3+6NO\rightarrow5N_2+6H_2O$
Bacteria will cause ammonia $NH_3$ to react with NO to put nitrogen back in the air, along with water, as part of the nitrogen cycle. If there are 3.56 moles of NO in the soil, how many moles of ammonia are needed to react with it?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{4\ mole\ NH_3}$

b)

$\frac{2\ mole\ NH_3}{3\ mole\ NO}$

c)

$\frac{6\ mole\ Hg}{5\ mole\ N_2}$

127.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation.... $4NH_3+6NO\rightarrow5N_2+6H_2O$
How many moles of water will be produced with 3.56 moles of NO in the soil?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{6\ mole\ H_2O}$

b)

$\frac{1\ mole\ H_2O}{1\ mole\ NO}$

c)

$\frac{6\ mole\ H_2O}{5\ mole\ N_2}$

128.

What is a limiting reactant?

a)

the reactant that determines how much product can be made

b)

the reactant that is in excess

c)

the product that you can make the most of

d)

the amount of reactants that react with each other

129.

You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich. If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?

a)

bread

b)

jelly

c)

peanut butter

d)

sandwich

130.

When 12 moles of O₂ reacts with 1.1 mole of C₁₀H₈what is the limiting reactant? C₁₀H₈ + 12 O₂ --> 10 CO₂ + 4 H₂O

a)

Oxygen

b)

C₁₀H₈

c)

Water

d)

Carbon Dioxide

131.

Use the equation 2 Al + 3 Cl₂ ---> 2 AlCl₃. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl3

b)

Cl2

c)

Al

132.

CH₄ + 2H₂O --> CO₂+ 4H₂What is the limiting reactant when 20g CH₄react with 15g H₂O?

a)

CH₄

b)

H₂O

c)

CO₂

d)

H₂

133.

Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?

a)

Fe

b)

S

c)

FeS

d)

none

134.

SO₂+ PCl₅--> SOCl₂+ POCl₃
How much SOCl₂is produced when 16.2g SO₂react with 13.7g PCl_5?

a)

7.87g

b)

30.1g

c)

26.4g

d)

19.8g

135.

The limiting reactant

a)

slows the reaction down

b)

is used up first

c)

is the reactant that is left over

d)

controls the speed of the reaction

136.

Use the equation 2 Al + 3 Cl₂ ---> 2 AlCl₃. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl₃

b)

Cl₂

c)

Al

137.

When does a chemical reaction stop?

a)

When the lab is finished

b)

When the excess reactant is used up

c)

When the limiting reactant is used up

d)

Chemical reactions never stop

138.

What is the limiting reactant if 10 moles of NH₃ react with 30.0 moles of NO?
4NH₃+6NO --> 5N₂ + 6H₂O

a)

NH₃

b)

NO

c)

N₂

d)

water

139.

P₄+ 3O₂--> P₄O₆
What is the limiting reactant is 12 moles of P₄react with 15 moles of O₂?

a)

P₄

b)

O₂

c)

P₄O₆

d)

none of the above

140.

4NH₃+ 5O₂--> 4NO + 6H₂O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen?

a)

0.37g

b)

0.045g

c)

1.35g

d)

11.1g

141.

Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?

a)

Fe

b)

S

c)

FeS

d)

none

142.

2 NaCl + Pb(NO₃)₂ --> 2 NaNO₃ + PbCl₂

How many grams of lead II chloride are produced from the reaction of 15.3 g of NaCl and 60.8 g of Pb(NO₃)₂?

a)

21.5g

b)

51.1g

c)

43.4g

d)

36.4g

143.

2Al + 3H₂SO₄ -> Al₂(SO₄)₃ + 3H₂
How many grams of aluminum sulfate would be formed if 250g H₂SO₄ completely reacted with aluminum?

a)

0.85 g

b)

290 g

c)

450 g

d)

870 g

144.

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

a)

Percent

b)

actual

c)

stoichiometry

d)

theoretical

145.

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

146.

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

a)

1.16%

b)

116%

c)

85%

d)

76%

147.

In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?

a)

82%

b)

0.82%

c)

10.1 %

d)

100%

148.

Reactant and products might adhere to containers causing actual yield to be less than theoretical yield.

a)

true

b)

false

149.

Competing reactions might occur forming other products causing your actual yield to be less than your theoretical yield.

a)

true

b)

false

150.

Some product can be transformed completely into energy causing your actual yield to be less than your theoretical yield.

a)

true

b)

false

151.

Some product may be lost during filtering causing your actual yield to be less than your theoretical yield.

a)

true

b)

false

152.

What is the equation to calculate percent yield?

a)

(Actual yield / Theoretical yield) x 100% = Percent yield

b)

(Theoretical yield / Actual yield) x 100% = Percent yield

c)

Mass (1 Mole / Molar mass) x 100% = Percent yield

d)

Mass x Speed x 100% = Percent yield

153.

Na₂CO₃+ 2HCl <=> 2NaCl + CO₂ + H₂O

Billy performed the preceding chemical reaction using 76g of Na₂CO₃ and produced 48g of NaCl. This did not match his theoretical yield. What was Billy's percent yield?

a)

50%

b)

22%

c)

48%

d)

57%

154.

Zn + 2HCl <=> ZnCl₂ + H₂

Billi performs the preceding reaction using 50g of Zinc and produced 10g of Zinc chloride. What is Billi's percent yield?

a)

42%

b)

36%

c)

24%

d)

30%

155.

What does percent yield indicate?

a)

The mass of product that should be obtained

b)

How quickly the reaction is completed

c)

The product of product actually obtained

d)

The efficiency of the chemical reaction

156.

Which of the following is NOT a reason for the actual yield to be different from the theoretical yield?

a)

some product is lost in purification

b)

more excess reactant is added

c)

competing reactions may use up reactants

d)

the limiting reactant may not be 100% pure

157.

A chemical reaction was carried out where a yield of 73g was expected, but a yield of 62g was obtained. Calculate the percent yield.

a)

85%

b)

118%

c)

84.9%

d)

11%

158.

What is an excess reactant?

a)

Substance you end with

b)

Substance that determines the rate of reaction

c)

Substance that is not used up completely

d)

Substance that is used up completely

159.

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

107%

c)

96.2%

d)

1.8%

160.

2. True or False?
A chemical reaction stops before the limiting reagent is used up.

a)

True

b)

False

161.

1. What is a limiting reagent?

a)

any reactant used up first in a reaction.

b)

any reactant left over at the end of a reaction.

c)

the maximum amount of product formed from a given amount of reactant.

d)

the purity of the reactant.

162.

7. The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.

a)

actual

b)

theoretical

c)

percent

163.

Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?

a)

25.2 grams

b)

37.3 grams

c)

37.1 grams

d)

36.3 grams

164.

What type of reaction is shown in the reaction pathway?

a)

endothermic reaction

b)

exothermic reaction

165.

What does all our work, provides all our heat, can be stored to use later, and never, ever goes away?

a)

enthalpy

b)

energy

c)

our best friend

d)

chemical bonds

166.

What are the two ways that internal energy can be transferred?

a)

by pressure, or by volume change

b)

by conduction, or by convection

c)

by heat, or by work

d)

by radiation, or by absorption

167.

Work is energy transferred to the motion of ___

a)

particles

b)

atoms and molecules

c)

objects

d)

humans

168.

Heat is energy transferred to the motion of ___

a)

trebuchets

b)

atoms and molecules

c)

objects

d)

nuclear particles

169.

What state function is based on the loss or gain of heat in a chemical reaction?

a)

energy

b)

enthalpy

c)

entropy

d)

volume

170.

Which letter is used to represent enthalpy in an equation?

a)

capital Q

b)

lowercase t

c)

capital H

d)

lowercase e

171.

Change in enthalpy is equal to ___

a)

pressure-volume work

b)

pressure on the Earth's surface

c)

the heat gained or lost by the system

d)

the internal energy of the system

172.

When a reaction takes place and enthalpy changes, that heat is transferring into or out of ___

a)

chemical bonds

b)

the nuclei of atoms

c)

a hand warmer

d)

newly created particles

173.

What type of chemical reaction releases energy through light or heat?

a)

an endothermic reaction

b)

an exothermic reaction

c)

an isothermic reaction

d)

an isobaric reaction

174.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

175.

_____ reactions usually feel hot!

a)

endothermic

b)

exothermic

176.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

177.

Endo means in or _______.

a)

absorbed

b)

released

178.

Exo means out or ________.

a)

absorbed

b)

released

179.

Exo means out or ________.

a)

absorbed

b)

released

180.

What instrument would you use to detect an endothermic or exothermic reaction?

a)

triple beam balance

b)

ruler

c)

thermometer

181.

HCl reacts with Zn giving off heat

a)

endothermic

b)

exothermic

182.

Surrounding temperature gets warmer

a)

endothermic

b)

exothermic

183.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

184.

What is the Heat of Reaction $\Delta H$ for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

185.

What is the potential energy of the products?

a)

40 kJ

b)

20 kJ

c)

100 kJ

d)

60 kJ

186.

What is the potential energy of the reactants?

a)

40 kJ

b)

20 kJ

c)

100 kJ

d)

60 kJ

187.

Is this reaction endothermic or exothermic?

a)

Endothermic

b)

Exothermic

188.

Is the reaction endothermic or exothermic?

a)

Endothermic

b)

Exothermic

189.

Is the reaction endothermic or exothermic?

a)

Endothermic

b)

Exothermic

190.

Which letter represents the products?

a)

B

b)

A

c)

Z

d)

X

191.

Which letter represents the reactants?

a)

B

b)

A

c)

Z

d)

X

192.

What is the activation energy?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

193.

What is the activation energy?

a)

30 kJ

b)

10 kJ

c)

40 kJ

d)

20 kJ

194.

Which letter represents the activation energy?

a)

B

b)

E

c)

C

d)

D

195.

Which number represents the activation energy?

a)

1

b)

2

c)

3

d)

4

196.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

197.

What is the heat of the reaction (ΔH)?

a)

250 kJ

b)

75 kJ

c)

225 kJ

d)

150 kJ

198.

Which letter represents the change of the heat of the reaction?

a)

B

b)

E

c)

C

d)

D

199.

Which number represents the change of the heat of the reaction (ΔH)?

a)

1

b)

2

c)

3

d)

4

200.

Which letter represents the location on the graph where the activated complex can be found?

a)

A

b)

B

c)

C

d)

D

201.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

202.

Is this reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

203.

What is the sign of ΔH for all endothermic reactions?

a)

Positive

b)

Negative

204.

What letter represents ΔH?

a)

A

b)

B

c)

C

d)

D

205.

What is the activation energy?

a)

40 kJ

b)

20 kJ

c)

100 kJ

d)

60 kJ

206.

What is the change of the heat of the reaction (ΔH)?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

207.

What is the PE of the reactants?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

208.

What is the PE of the products?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

209.

What is the activation energy?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

210.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

211.

What letter represents the energy of the products?

a)

A

b)

B

c)

C

d)

D

212.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

213.

What is the activation energy?

a)

40 kJ

b)

20 kJ

c)

100 kJ

d)

60 kJ

214.

Which letter represents the activation energy?

a)

B

b)

E

c)

C

d)

D

215.

What is the sign of ΔH for all endothermic reactions?

a)

Positive

b)

Negative

216.

What is the change of the heat of the reaction (ΔH)?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

217.

What is the PE of the products?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

218.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

219.

What letter represents the activation energy for the forward reaction?

a)

A

b)

B

c)

C

d)

D

e)

E

220.

What letter represents the energy of the products?

a)

A

b)

B

c)

C

d)

D

221.

What letter represents the activation energy for the forward reaction?

a)

A

b)

B

c)

C

d)

D

e)

E

222.

Is the forward reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

223.

Is the forward reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

224.

What is the value of ΔH_rxn for the forward reaction?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

e)

20 kJ

225.

What is the PE of the products?

a)

100 kJ

b)

175 kJ

c)

50 kJ

d)

75 kJ

226.

The Universe tends toward ___

a)

order

b)

disorder

c)

harmony

d)

kindness

227.

Which law of thermodynamics says that "any spontaneous process increases the randomness of the Universe"?

a)

zeroth

b)

first

c)

second

d)

third

228.

The very act of putting one system in order requires that other systems become ___

a)

disordered

b)

ordered as well

c)

hotter

d)

colder

229.

For your lunch to give you energy, it has to be broken down into which less ordered nutrients?

a)

greases, fats, and lipids

b)

carbohydrates, sugars, and starches

c)

carbohydrates, proteins, and lipids

d)

proteins and amino acids

230.

The macronutrients from your lunch were broken down even further as they were converted to ___

a)

proteins

b)

energy in your cells

c)

starches

d)

polymers

231.

Cleaning your house in fact increases the overall disorder of ___

a)

your house

b)

your office

c)

your kitchen

d)

the Universe

232.

In chemistry, the measure of molecular randomness, or disorder, is dubbed ___

a)

entropy

b)

ethalpy

c)

disorderly

d)

Gibb's free energy

233.

The Second Law of Thermodynamics says that "any spontaneous process increases the ___"

a)

order of the Universe

b)

disorder of the Universe

c)

temperature of the system

d)

temperature of the surroundings

234.

"Spontaneous" simply means a process that doesn't need ___

a)

a spark to ignite it

b)

parental approval

c)

to be at a specific temperature

d)

outside energy to proceed

235.

Anything that increases the disorder of the Universe ___

a)

is not permitted

b)

happens spontaneously

c)

occurs instantly

d)

is exothermic

236.

Which letter is used to represent entropy in an equation?

a)

the capital letter "S"

b)

the capital letter "H"

c)

lowercase letter "q"

d)

lowercase letter "t"

237.

What is a reaction that absorbs heat from the surroundings called?

a)

an endothermic reaction

b)

an exothermic reaction

c)

a combustion reaction

d)

a precipitation reaction

238.

The enthalpy change of the reaction was found using Hess's Law and ___

a)

common entropies of creation

b)

Gibb's Law

c)

standard enthalpies of formation

d)

the van der Waals equation

239.

What does a positive value for the change in standard enthalpy indicate?

a)

the reaction absorbed thermal energy

b)

the reaction emitted thermal energy

c)

the reaction emitted radiation

d)

the reaction absorbed photons

240.

What does a positive value for the change in standard entropy mean?

a)

the products are more ordered than the reactants

b)

the products are more disordered than the reactants

c)

the reaction absorbed thermal energy

d)

the reaction emitted thermal energy

241.

Which letter is used to represent Gibbs free energy in an equation?

a)

capital "F"

b)

capital "G"

c)

lowercase "g"

d)

lowercase "f"

242.

If ΔG is positive, the reaction is ___

a)

not spontaneous

b)

spontaneous

c)

in an equilibrium state

d)

not discernible

243.

If ΔG is negative, the reaction is ___

a)

not spontaneous

b)

spontaneous

c)

in an equilibrium state

d)

undefined

244.

Reactions which do not produce the written products under the given conditions.

a)

spontaneous

b)

nonspontaneous

245.

Spontaneous reactions may be extremely slow.

a)

True

b)

False

246.

Nonspontaneous reactions may be extremely fast under the specified conditions.

a)

True

b)

False

247.

Two factors that determine the spontaneity of a reaction are:

a)

entropy and free energy

b)

enthalpy and free energy

c)

entropy and enthalpy

d)

endothermic and exothermic

248.

Reactions tend to be spontaneous if they are exothermic.

a)

True

b)

False

249.

Reactions tend to be spontaneous if the reactants have more energy than the products.

a)

True

b)

False

250.

Gases have more entropy than liquids.

a)

True

b)

False

251.

Solids have more entropy than liquids.

a)

True

b)

False

252.

An increase in numbers of moles from reactants to products (e.g. 3A --> 4 B) would cause a decrease in entropy.

a)

True

b)

False

253.

The release of energy from a reaction indicates an increase in entropy of the universe.

a)

True

b)

False

254.

For the following reaction indicate if entropy is increased or decreased. 2 Li(s) + 2 H₂O(l) ---->2 LiOH(s) + H₂(g) + 213.0 kJ (Kilojoules)

a)

increase

b)

decrease

255.

For the following reaction indicate if entropy is increased or decreased. 2N₂(g) + 3 H₂(g) -------> 2 NH₃(g)

a)

increase

b)

decrease

256.

For the following reaction indicate if entropy is increased or decreased. KClO₃(s) ------> KCl(s) + O₂(g)

a)

increase

b)

decrease

257.

Reactions are always spontaneous if they are exothermic, regardless of entropy change.

a)

True

b)

False

258.

Spontaneous reactions release free energy.

a)

True

b)

False

259.

The symbol for entropy is

a)

H

b)

S

c)

G

260.

The symbol for enthalpy is

a)

S

b)

H

c)

G

261.

A measure of the disorder of a system

a)

enthalpy

b)

entropy

c)

energy

d)

free energy

Chemistry Final Exam Review Units 7-9

Total questions: 261

Worksheet time: 22hrs 45mins

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