Free Printable Spring 2024 Review

1.

Neon occupies a volume of 2.80 L at -35°C. What volume will it occupy at 43°C?

a)

3.44 L

b)

4.1 L

c)

2.65 L

d)

3.7 L

2.

What is 50 C in Kelvin?

a)

223

b)

323

c)

100

d)

50

3.

Gas laws involve what three variables?

a)

Solid Liquid Gas

b)

Speed Velocity Acceleration

c)

Elements Compounds Mixtures

d)

Pressure Temperature Volume

4.

According to the Combined Gas Law, pressure and volume are inversely related which means that

a)

When pressure increases, volume increases

b)

When pressure decreases, volume decreases

c)

When pressure increases, volume decreases

d)

When pressure doubles, volume triples

5.

According to the Combined Gas Law, volume and temperature are directly related. This means that

a)

When volume increases, temperature increases

b)

When volume increases, temperature decreases

c)

When volume double, pressure triples

d)

When volume doubles, volume is reduced by 1/2

6.

If 6L of gas at 293K is compressed to 4L, what is the new temperature?

a)

195K

b)

439.5K

c)

0.082K

d)

12.2K

7.

4L of a gas is contained at 300 kPa and 200K. What will its volume be in L at 140 kPa and 100K?

a)

4.3L

b)

4.8L

c)

6.2L

d)

8.5L

8.

Using Combined Gas Law, if the pressure of a gas starts out at 200kPa and increases to 600kPa, what would the initial temperature be if it ended up at 300K?

a)

50K

b)

200K

c)

400K

d)

100K

9.

The energy of an object as it is in motion is defined as

a)

Kinetic Theory

b)

Kinetic energy

c)

Potential energy

d)

Electric energy

10.

When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the

a)

air molecules hit the walls of the tire less frequently

b)

rubber in the tires reacts with oxygen in the atmosphere

c)

air molecules speed up and collide with the tire walls more often

d)

air molecules diffuse rapidly through the walls of the tire.

11.

If the pressure in a balloon remains constant what happens to the balloon's volume as the temperature of the air increases?

a)

the volume decreases and the balloon shrivels up or shrinks

b)

the volume increases and the balloon expands

c)

the volume stays the same and the balloon stays the same size

12.

Each of the flasks shown above have different volumes (they are different sizes) but the temperature of each flask is the same. In which flask will the pressure be the highest?

a)

Flask 1

b)

Flask 2

c)

Flask 3

d)

Flask 4

13.

Which equation would you use to solve the following problem:

"The volume of of 300 mL of gas at 1 atm is decreased to 100 mL. What is the new pressure?"

a)

P₁V₁ = P₂V₂

b)

V₁/T₁ = V₂/T₂

c)

(P₁V₁)/T₁ = (P₂V₂)/T₂

d)

None of the above

14.

Which equation would you use to solve the following problem:

"A gas occupies 2 L of space at 0 C. What will its volume be at 100 C?"

a)

P₁V₁ = P₂V₂

b)

V₁/T₁ = V₂/T₂

c)

(P₁V₁)/T₁ = (P₂V₂)/T₂

d)

None of the above

15.

A tank of helium is full with a pressure of 4.5 atm at 298K. What is the temperature of the tank when the pressure drops to 2 atm?

a)

670.5K

b)

0.007K

c)

132.4K

d)

2682K

16.

1.70 atm, a sample of gas takes up 4.25L. If the pressure in the gas is increased to 2.40 atm, what will the new volume be?

a)

0.167 L

b)

6.00 L

c)

3.01 L

d)

0.332 L

17.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

18.

A student sprays perfume in the back of the classroom, eventually a student in the front of the class can smell the perfume. This is an example of....

a)

Effusion

b)

Diffusion

c)

Osmosis

d)

Thermal Expansion

19.

A container with a volume if 1.0 L is occupied by a gas at a pressure of 1.5 atm at 25°C. By changing the volume, the pressure of the gas increases to 6.0 atm as the temp is raised to 100.°C. What’s the new volume?

a)

1.45 L

b)

5.4 L

c)

0. 31 L

d)

504.7 L

20.

The pressure in an automobile tire is 2.3 atm at 27°C. At the end of a journey on a hot, sunny day the pressure has risen to 2.6 atm. What is the temp of the air in the time assuming the volume has not changed?

a)

60 K

b)

650 K

c)

273 C

d)

339 K

21.

What is the variable for V for idea gas laws

a)

mm Hg

b)

mL

c)

gallons

d)

L

22.

How can you convert from mL to L

(a)

23.

What is the variable for T ideal gas

a)

K

b)

^oC

c)

F

24.

How do you convert from ^oC to K

(a)

25.

What are the variables we can use for P in ideal gas

a)

mm HG

b)

kPa

c)

Pa

d)

atm

26.

What is the variable for n in ideal gas

a)

g

b)

mol

27.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

28.

Which is a correct unit for R?

a)

L.atm/mol.k

b)

L.atm

c)

mmHg/mol.K

d)

L.atom/mol

29.

What is the equation for Ideal Gas Law (hint what we have been studying)

(a)

30.

1 atm =

a)

760 mm Hg

b)

920 mm Hg

c)

102 mm Hg

d)

786 mm Hg

31.

1 atm =

a)

1829 kPa

b)

91.9 kPa

c)

101.3 kPa

d)

111.3 kPa

32.

What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT

a)

14.19 atm

b)

16.53 atm

c)

18.42 atm

d)

22.54 atm

33.

If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?

a)

.002766 mole

b)

.0069 mol

c)

2.766 mol

d)

9.887 mol

34.

Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.

a)

0 K

b)

107 K

c)

207 K

d)

307 K

35.

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.

a)

7.18 L

b)

7.81 L

c)

4.63 L

d)

4.36 L

36.

The specific heat of aluminum is 0.21 cal/g°C. How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

a)

105 J

b)

10.5 J

c)

1.05 J

37.

20 g of water. specific heat of water is 4.18 J/x°C. temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?

a)

418 Joules

b)

209 J

c)

83 J

d)

4.18 J

38.

A material was cooled from 100ºC to 40ºC. What is the temperature change?

a)

60ºC

b)

40ºC

c)

-60ºC

d)

-40ºC

39.

The specific heat of aluminum is 0.21 cal/g°C. How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

a)

105 J

b)

10.5 J

c)

1.05 J

40.

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

351 °C

41.

The specific heat is the amount of energy needed to raise the temperature one degree Celsius of a substance.

a)

True

b)

False

42.

Calculate the heat needed to raise the temperature of 0.25 kg of aluminum 7°C (c=900 J/kg°C)

a)

1575 J

b)

-1575 J

c)

514 J

d)

-514 J

43.

The amount of energy required to raise the temperature 1ºC for every kilogram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

44.

Water has a specific heat of 4184 J/KgºC. Wood has a specific heat of 1760 J/KgºC. What material needs more energy to raise the temperature 1ºC

a)

Wood

b)

Water

c)

Both are the same

45.

How does heat flow?

a)

Always from cold to warm

b)

Always from warm to cold

c)

Both warm to cold & cold to warm

d)

It depends on the temperature

46.

When a piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?

a)

50°

b)

0°

c)

100°

d)

150°

47.

A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils (100˚C). The specific heat of water is 4.18 J/(g˚C).
Determine the heat energy needed to heat the water in the pot to boiling.

a)

133.76J

b)

43,062.2J

c)

752,400J

d)

1,003,200J

48.

The temperature of an unknown piece of metal with a mass of 30.00 g changes from 25.0 °C to 35.0 °C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?

a)

1.17 J/g°C

b)

-1.17 J/g°C

c)

0.857 J/g°C

d)

-0.857 J/g°C

49.

How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?

a)

1476 J

b)

2926 J

c)

210,050 J

d)

1,404,500 J

50.

Use the information in the image to answer this question.

The standard enthalpy of combustion of butane, in kJ mol⁻¹, is

a)

−2880

b)

−2590

c)

−806

d)

−554

51.

Use the information in the image to answer this question.

The value in kJ mol⁻¹ of the enthalpy of thermal dissociation when butane forms propane, hydrogen and carbon is

a)

−26.3

b)

−17.5

c)

+17.5

d)

+21.2

52.

Use the information in the image to answer this question.

The value in kJ mol−1 for the enthalpy of combustion of propane is

a)

−211.7

b)

−419.7

c)

−2220

d)

−2878

53.

Using the data below, which is the correct value for the standard enthalpy of formation for TiCl₄(l)?

a)

−1538 kJ mol⁻¹

b)

−1094 kJ mol⁻¹

c)

−750 kJ mol⁻¹

d)

+286 kJ mol⁻¹

54.

The enthalpies of combustion of C(s), H2(g) and C4H9OH(l) (in kJmol^-1) are as follows
C(s) + O₂(g) -> CO₂(g) ∆H=a
H₂(g) + ½O₂(g) -> H₂O(l) ∆H=b
C₄H₉OH(l) + 6O₂(g) -> 4CO₂(g) + 5H₂O(l) ∆H=c
What is the enthalpy change for the reaction shown below?
4C(g) + 5H₂(l) + ½O₂(g) -> C₄H₉OH(l)

a)

c – 4a – 5b

b)

2a + 10b - c

c)

4a + 5b - c

d)

2a + 5b + c

55.

(Hess's Law)Calculate the ∆H for the following reaction: 2H₂O₂→ 2H₂O + 1 O₂
You are given these two equations:
2H₂+ O₂ → 2H₂O ∆H = -572 kJ
H₂ + O₂→ H₂O₂ ∆H = -188 kJ

a)

∆H = -948 kJ

b)

∆H = -196 kJ

c)

∆H = -384 kJ

d)

∆H = -188 kJ

56.

When you multiply a chemical equation by 2, what is done to the heat of reaction?

a)

multiplied by 1/2

b)

multiplied by 2

c)

nothing

57.

When you flip a chemical reaction using Hess's Law, what is done to the heat of reaction value?

a)

nothing

b)

the sign is flipped

c)

1/delta H

58.

Solutions that conduct a current are called ____________ and are made from ___________ compounds.

a)

electrolytes; ionic

b)

nonelectrolytes; ionic

c)

electrolytes; molecular

d)

electrolytes; covalent

59.

Oil molecules are nonpolar. What kind of solvent is required to remove an oil stain?

a)

saturated

b)

unsaturated

c)

polar

d)

nonpolar

60.

True or false:

Dissolved particles will pass through a piece of filter paper.

a)

True

b)

False

61.

Which of the following is NOT a solution?

a)

the air you breathe

b)

carbonated soda

c)

nail polish mixed with acetone

d)

milk

62.

Which of the following has the MOST surface area?

a)

A single 5 gram ice cube

b)

5 grams of crushed ice

c)

5 grams of shaved ice

63.

You begin with a solution of 400 grams of potassium chloride dissolved in 1250 mL of water. If the volume of water is increased by 33%, what is the final molarity of the solution?

a)

3.2 M

b)

4.3 M

c)

5400 M

d)

5.4 M

64.

If 400 mL of a 8.0 M solution is diluted to a molarity of 5.3M, about how much solvent volume was added?

a)

200 mL

b)

600 mL

c)

400 mL

d)

180 mL

65.

This solution would be considered

a)

Unsaturated

b)

Supersaturated

c)

Saturated

d)

Undefined

66.

An electrolyte is...

a)

The rapid, random movement of particles in colloidal dispersion.

b)

A substance that dissolves in water and conducts electric current.

c)

A substance that dissolves in water and does not conduct electric current.

d)

The solution process when water is the solvent.

67.

The ___ is the thing being dissolved.

a)

solute

b)

solvent

c)

mixture

d)

suspension

68.

You and your friend have a contest to see who can make sweet iced tea the fastest. Which of the following would NOT help you win?

a)

Cooling the water

b)

Using smaller sugar crystals

c)

Heating the water

d)

Stirring quickly

69.

amount of solute that can dissolve in a given amount of solvent at a given temperature

a)

saturated solution

b)

solubility

c)

pure substance

d)

colloid

70.

what is the molarity of a solution that contains 125 g NaCl in 4.00 L of solution?

a)

0.535 M NaCl

b)

2.14 M NaCl

c)

8.56 M NaCl

d)

31.3 M NaCl

71.

A dissolved solute that does not form ions is:

a)

a nonelectrolyte

b)

a weak electrolyte

c)

a strong electrolyte

d)

insoluble

72.

What is the most common solvent in everyday life?

a)

Ethanol

b)

Tuluene

c)

Water

d)

Oils

73.

How does temperature affect solubility?

a)

Solubility is not affected by temperature.

b)

Solubility decreases with an increase in temperature.

c)

Solubility increases with an increase in temperature.

74.

air is a

a)

compound

b)

element

c)

heterogeneous mixture

d)

solution

75.

When you make a dilution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

76.

How do we make a dilution?

a)

Add more solute

b)

Remove solute

c)

Remove solvent

d)

Add more solvent

77.

A solution that has water as the solvent is called a(n).....

a)

Aqueous Solution

b)

Water-Based Solution

c)

Organic Solution

d)

Dilute Solution

78.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

79.

What is the molarity of a solution containing 400 g of CuSO₄ (FM: 159.6 g/mol) in 4.0 L of solution?

a)

100 M

b)

1.6 M

c)

0.626 M

d)

0.01 M

80.

How many moles of solute are present in 50.0 mL of 0.20M KNO₃?

a)

10.0 moles solute

b)

0.05 moles solute

c)

1.00 moles solute

d)

0.01 moles solute

81.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

82.

How many mL of 1.0M KBr solution would you need to prepare 250 mL of a 0.2M dilution?

a)

175 mL

b)

250 mL

c)

50 mL

d)

5 mL

83.

What would the molarity of a solution be if you took 10 mL of a 13M stock solution and made a 300 mL solution?

a)

390M

b)

230M

c)

0.43M

d)

0.26M

84.

You are adding a chlorine solution to a swimming pool. The stock solution of chlorine is 1000M. Your swimming pool (75,000 L) needs to be at a concentration of 0.1M. How much of the stock solution should you add?

a)

7500 L

b)

.75 L

c)

750 L

d)

7.5 L

85.

The smallest unit of matter in the universe is the __________.

a)

molecule

b)

compound

c)

atom

d)

does it really matter?

86.

All of the following are subatomic particles, EXCEPT:

a)

proton

b)

compound

c)

electron

d)

neutron

87.

The number of protons an atom has is its _________ number.

a)

neurotic

b)

covalent

c)

ionic

d)

atomic

88.

A(n) __________________ is an atom that has the same number of protons and electrons but different numbers of neutrons.

a)

isotope

b)

ion

c)

compound

d)

molecule

89.

A(n) ______________ is an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

a)

bond

b)

ion

c)

isotope

d)

molecule

90.

A(n) __________________ in a positively charges atom.

a)

anion

b)

cation

c)

onion

d)

isotope

91.

_____________________ is a substance made up of 2 or more different types of atoms.

a)

A compound

b)

An isotope

c)

An ion

d)

A bond

92.

A(n) _____________________ is the smallest amount of a compound you can have, and still have that compound.

a)

atom

b)

smidgen

c)

proton

d)

molecule

93.

A bond created by a transferring of electrons from one atom to another is called a(n) _______________ bond.

a)

transferric

b)

covalent

c)

ionic

d)

lovely

94.

A bond created by atoms sharing 1 or more electrons is called a(n) _______________________ bond.

a)

moronic

b)

covalent

c)

ionic

d)

isotonic

95.

Solutions that have more OH– ions than H+ ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

96.

Solutions that have more H+ ions than OH- ions are

a)

acids

b)

bases

c)

enzymes

d)

neutral

97.

Which of the following is the strongest acid?

a)

soap - 10

b)

HCL - 0

c)

blood - 7.45

d)

soft drink - 3

98.

Which of the following is the strongest base?

a)

soap - 10

b)

HCL - 0

c)

blood - 7.45

d)

soft drink - 3

99.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

100.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

101.

When acids react with metals, they produce hydrogen gas and salt.

a)

True

b)

False

102.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

103.

Which of the following is an acid?

a)

vinegar

b)

bleach

c)

sugar in water

d)

starch in water

e)

toothpaste in water

104.

The pH value of an acid represents its __________ of positive ions in the solution

a)

amount

b)

concentration

c)

color

d)

charge

105.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

106.

Bases have many uses. They are mainly used to make

a)

cleaning products

b)

soaps

c)

concrete

d)

all of the answer choices

107.

Bases turn blue litmus paper red.

a)

True

b)

False

108.

Turns litmus red

a)

Acids

b)

Bases

c)

All

109.

Which has a slippery texture?

a)

Acid

b)

Base

110.

Plaster of Paris is made from

a)

Lime stone

b)

Slaked Lime

c)

Quick lime

d)

Gypsum

111.

Setting of Plaster of Paris takes place due to

a)

Oxidation

b)

Reduction

c)

Dehydration

d)

Hydration

112.

Washing soda has the formula

a)

Na2CO3.7H2O

b)

Na2CO3.10H2O

c)

Na2CO3.H2)

d)

Na2CO3

113.

BASE + ACID ----> SALT +?

a)

water

b)

oxygen

c)

hydrogen ion

d)

hydroxide ion

114.

What is the name of this ion: H₃O⁺?

a)

helium ion

b)

hydrogen ion

c)

hepatic ion

d)

hydronium ion

115.

A drop of solution 'X' is placed on a strip of pH paper. A deep red colour is produced. The solution 'X' is

a)

NaOH

b)

HCl

c)

H₂O

d)

Na₂CO₃

116.

Which of the following base is used in the manufacture of bleaching powder?

a)

Sodium hydroxide

b)

Calcium hydroxide

c)

Potassium hydroxide

d)

Magnesium hydroxide

117.

A colourless and odourless gas is liberated when hydrochloric acid is added to a solution of washing soda. The name of the gas is

a)

Carbon dioxide

b)

Nitrogen dioxide

c)

Sulphur dioxide

d)

Sulphur trioxide

118.

The compounds obtained on heating baking soda are

a)

Sulphur dioxide and sodium carbonate

b)

Sodium bicarbonate, water and carbon dioxide

c)

Sodium carbonate, water and carbon dioxide

d)

Hydrochloric acid and water

119.

A ___ is formed when an positive ion bonds with a negative ion.

a)

Acid

b)

base

c)

salt

d)

neutral ion

120.

What should go in the question mark spot?

$57.2\ grams\ NiS\ \times\ \frac{1\ mol}{?}=0.63\ mol$

a)

$6.02x10^{23}\ mc$

b)

1 mole

c)

90.75 grams

d)

57.2 grams

121.

If you start with $8.47x10^{24}\ molecules$ , how many conversion fractions does it take to convert to grams?

a)

1

b)

2

122.

How many moles are in $3.92x10^{23}$ molecules of $CaF_2$ ?

Which part of the setup is incorrect?

$3.92x10^{23}\ molecules\ \times\ \frac{1\ mole}{78.08\ g}$

a)

$3.92x10^{23}\ molecules$

b)

1 mole

c)

78.08 g

123.

How many grams are in $9.28x10^{23}\ molecules$ of NaCl?

Choose the correct setup.

a)

$9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ grams}{1\ mole}$

b)

$9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ mc}{1\ mole}\times\frac{58.44\ g}{1\ mole}$

c)

$9.28x10^{23}\ molecules\ \times\frac{1\ mole}{6.02x10^{23}\ mc}\times\frac{58.44\ g}{1\ mole}$

d)

$9.28x10^{23}\ molecules\ \times\frac{58.44\ g}{1\ mole}$

124.

How many grams are in 2.9 moles of $SiCl_4$ ? Fill in the missing information.

$2.9\ mol\ \times\ \frac{?\ grams}{1\ mole}=492.68\ g\ SiCl_4$

(a)

125.

How many molecules are in 4.93 moles of $Ga_2S_3$ ? Fill in the missing information.

$4.93\ mol\ \times\ \frac{?\ molecules}{1\ mole}$

(a)

126.

If you're starting with $7.31x10^{24}\ molecules$ of SrS and you want to convert to moles, what would go on the bottom of the conversion fraction?

$7.31x10^{24}\ molecules\ \times\frac{ }{??????????????}$

a)

$6.02x10^{23}\ molecules$

b)

1 mole

c)

119.68 g

127.

What is the molar mass of Al₂(CO₃)₃?

a)

113.97 g/mol

b)

137.99 g/mol

c)

233.99 g/mol

d)

185.99 g/mol

128.

If you have 82.21 grams of NO₂, how many molecules do you have?

Pick the correct setup.

a)

$82.21\ g\ \times\frac{1\ mol}{46.01\ g}\times\frac{1\ mol}{6.02x10^{23}\ molecules}$

b)

$82.21\ g\ \times\frac{1\ mol}{46.01\ g}\times\frac{6.02x10^{23}\ molecules}{1\ mol}$

c)

$82.21\ g\ \times\frac{6.02x10^{23}\ molecules}{1\ mol}$

d)

$82.21\ g\ \times\frac{1\ mol}{46.01\ g}$

129.

How many moles are in 2.67x10²⁴ molecules of H₂O?

What is the missing piece?

$2.67x10^{24}\ molecules\times\frac{???????????}{6.02x10^{23}\ mc}$

a)

6.02x10²³ mc

b)

1 mole

c)

18.016 grams

d)

2.67x10²⁴ mc

130.

If you're starting with 82.21 grams of PH₃ and you want to convert to moles, what would go on the bottom of the conversion fraction?

$82.21\ grams\ \times\frac{ }{??????????????????}$

a)

1 mol

b)

33.994 grams

c)

6.02x10²³ mc

d)

82.21 grams

131.

How many Carbons "C" are in C₁₈H₃₄O₃

a)

18

b)

34

c)

3

d)

37

132.

What is the best definition for subscript?

a)

The big number that tells you the number of molecules.

b)

The atomic number

c)

The little number that tells the number of atoms for each element.

133.

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

a)

Mg₄N₃

b)

MgN₂

c)

Mg₃N₂

d)

MgN

134.

Molecular Formula = C₂F₆

Choose the correct empirical formula.

a)

CF

b)

C₂F₆

c)

C₃F

d)

CF₃

135.

Which pair has the same empirical formula?

a)

NaCrO₄ and Na₂Cr₂O₇

b)

C₂H₄O₂ and C₆H₁₂O₆

c)

C₃H₆O₃and C₂H₆O₂

d)

CH₄ and C₂H₆

136.

Empirical Formula = CF₂

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C₄F₈

b)

C₈F₄

c)

C₃F₆

d)

C₂F₄

137.

Molecular Formula = Si₂F₆

Choose the correct empirical formula.

a)

SiF

b)

Si₂F₆

c)

SiF₃

d)

Si₄F₁₂

138.

How would you calculate the molar mass for C₄H₆?

a)

12.0111 + 1.00794

b)

4(12.0111) + 6(1.00794)

c)

2(12.0111) + 3(1.00794)

d)

6(12.0111) + 4(1.00794)

139.

The empirical formula of a substance is CH₂O. The molar mass is 180g/mol. What is the molecular formula?

a)

CH₂O

b)

C₃H₆O₃

c)

C₆H₁₂O₆

d)

C₁₂H₆O₁₂

140.

What is the empirical formula of K₂SO₄?

a)

K₂SO₄

b)

KSO₂

c)

K₂SO₂

d)

KSO₈

141.

What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

142.

A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________

a)

ionic formula

b)

covalent formula

c)

empirical formula

d)

molecular formula

143.

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

144.

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

145.

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

146.

In this image, what are the information in red is called the_______.

a)

Product

b)

Reactant

c)

Chemical Subscript

d)

Yield

147.

In this image, what are the information to the right of the arrow (in black) is called the_______.

a)

Product

b)

Reactant

c)

Chemical Subscript

d)

Yield

148.

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

149.

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

150.

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

151.

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

152.

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

Spring 2024 Review

Total questions: 152

Worksheet time: 8hrs 45mins

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