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Chemistry Spring Final Exam Review

Total questions: 80

Worksheet time: 3hrs 52mins

Name
Class
Date
1.

What do you use when converting from moles of Fe to atoms of Fe?

a)

Coefficient Ratio

b)

Avogadro's Number

c)

Molar mass

d)

Conservation of Mass

2.
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
3.
How many grams are in 7.8 moles of NaCl?
a)

476 grams

b)

460 grams

c)

452 grams

d)

462 grams

4.

B2H6 + 3 O2 -->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

5.

4 Al + 3 O2 –> 2 Al2O3 How many moles of aluminum would be needed to completely react with 45 grams of O2?

a)

1.05 moles

b)

3.75 moles

c)

1.875 grams

d)

1.875 moles

6.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
7.

In a chemical reaction, the mass of reactants ___.

a)

is less than the mass of products

b)

is greater than the mass of products

c)

has no relationship to the mass of products

d)

is equal to the mass of products

8.
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
9.

What is the limiting reactant if 10 moles of NH3 react with 16.0 moles of NO?

4 NH3 + 6 NO --> 5 N2 + 6 H2O

a)

LR: NH3 and ER: 1 mol NO

b)

LR: NO and ER: 1 mol NH3

c)

LR: NH3 and ER: 2 mol NO

d)

LR: NO and ER: 2 mol NH3

10.

P4 + 3 O2 --> P4O6

What is the limiting reactant is 3 moles of P4 react with 8 moles of O2?

a)

LR: P4 and ER: 0.33 mol O2

b)

LR: O2 and ER: 0.33 mol P4

c)

LR: P4 and ER: 0.67 mol O2

d)

LR: O2 and ER: 0.67 mol P4

11.

What best explains why a student might end up with a percent yield of over 115%?

a)

Actual yield is too large; contamination

b)

Actual yield is too small; spilt product

c)

Actual yield is too large; spilt product

d)

Actual yield is too small; contamination

12.

What do you use when converting from moles of Fe to grams of Fe?

a)

Coefficient Ratio

b)

Avogadro's Number

c)

Molar mass

d)

Conservation of Mass

13.

What do you use when converting from moles of Fe to moles of FeCl2?

a)

Coefficient Ratio

b)

Avogadro's Number

c)

Molar mass

d)

Conservation of Mass

14.

How many molecules of H2O are in 4 moles of H2O? 

a)

6.02 x 1023

b)

8

c)

4

d)

2.4 x 1024

15.

How many atoms of H are in 4 molecules of H2O? 

a)

6.02 x 1023

b)

8

c)

4

d)

2.4 x 1024

16.

Heat is measured in

a)

Joules

b)

Grams

c)

degrees Celsius

d)

Joules per gram Celsius

17.

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change (∆T) when 100 Joules of heat ( ΔH\Delta H )  is added to 10 grams?

a)

0.0039 °C

b)

3.9 °C

c)

390 °C

d)

25.64 °C

e)

-3.9 °C

18.
Thermal energy always moves:
a)
From a high temperature object to a lower temperature object.
b)
From a lower temperature object to a higher temperature object.
c)
From an object with lower kinetic energy to an object with higher kinetic energy.
d)
From an object of higher mass to an object of lower mass.
19.

The temperature of a glass of cold water will eventually...

a)

Equal the temperature of the surrounding environment.

b)

Always be colder than the surrounding environment.

c)

Become warmer than the surrounding environment.

d)

Never change temperature.

20.

A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH\Delta H  .

a)

endothermic; positive

b)

endothermic; negative

c)

exothermic; negative

d)

exothermic; positive

21.

The specific heat (c) of platinum is 0.13 J/g °C. What heat ( ΔH\Delta H  ) is needed to raise a 5 g ring 15 °C?

a)

576.9 J

b)

-576.9 J

c)

2.56 J

d)

23.1 J

e)

9.75 J

22.

A cold pack is placed on Karl's head after he is elbowed during a wrestling match. _____ Energy will be transferred from _______

a)

Cold; pack to head

b)

Heat; pack to head

c)

Cold; head to pack,

d)

Heat; head to pack

23.

Which metal would increase temperature the fastest?

a)

Zn, lowest specific heat

b)

Cu, lowest specific heat

c)

Sn, lowest specific heat

d)

Mn, highest specific heat

e)

Si, highest specific heat

24.

Ammonium nitrate is added to water in a plastic bag. You feel the outside of the bag and it turns really cold. The reaction IN the bag is _________________.

a)

Exothermic, absorbing heat from the surroundings

b)

Endothermic, absorbing heat from the surroundings

c)

Exothermic, releasing heat to the surroundings

d)

Endothermic, releasing heat to the surroundings

25.

Energy needs to be _____________ to break bonds and ____________ to form bonds.

a)

absorbed; released

b)

absorbed; absorbed

c)

released; released

d)

released; absorbed

26.

What is the activation energy (EA) of the reaction?

a)

250 kJ

b)

100 kJ

c)

200 kJ

d)

150 kJ

e)

50 kJ

27.

Eventually all the clothes in your closet will end up on the floor because _____.

a)

Enthalpy tends to increase

b)

Entropy tends to increase

c)

Enthalpy tends to decrease

d)

Entropy tends to decrease

28.

A physical change of solid ice to liquid water is ___________.

a)

exothermic and increases entropy

b)

endothermic and increases entropy

c)

exothermic and decreases entropy

d)

endothermic and decreases entropy

29.

The following reaction: 2 H2 (g) + O2 (g) --> 2 H2O (g) _____ entropy because _________ moles produced.

a)

increases; less

b)

decreases; less

c)

increases; more

d)

decreases; more

30.

Systems in nature tend to undergo changes toward

a)

lower energy and less disorder

b)

lower energy and more disorder

c)

higher energy and less disorder

d)

higher energy and more disorder

31.

Consider the following equations.


Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ


What is the ∆H value (in kJ) for the following reaction?


MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

32.

Determine the entropy of the following reaction of PCl5 (g) --> PCl3 (g) + Cl2 (g) given that

So PCl5 (g) = 364.2 J/molK

So PCl3 (g) = 311.6 J/molK

So Cl2 (g) = 223.1 J/molK

a)

  • - 452.7 J/K

b)

  • + 452.7 J/K

c)

  • + 170.5 J/K

d)

  • - 170.5 J/K

33.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

34.

What is a spontaneous process ?

a)

slow process

b)

fast process

c)

process that needs an external intervention to occur

d)

process that does not need external intervention to occur / keep happening

35.

Which combination of ΔH and ΔS ALWAYS results in a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

36.

2 Pb(NO3)2 --> 2 PbO + 4 NO2 + O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

37.
2Fe + 3H2SO4 --> Fe2(SO4)3 + 2H2
a)
Synthesis 
b)
Decomposition
c)

Single 

Replacement

d)
Combustion
38.

Using the activity series, Li + NiNO3 -->

a)

Ni + Li(NO3)2

b)

NO3 + LiNi

c)

LiNiNO3

d)

No Reaction

39.

In single replacement reactions .............

a)

Metals replace nonmetals

b)

Nonmetals replace metals

c)

metals replace metals

d)

nonmetals replace nonmetals

40.

Precipitates occur when a(n) ____________ forms.

a)

Soluble compound

b)

Insoluble compound

c)

soluble or insoluble compound

d)

gas

41.

When Mg is added to HCl, Mg replaces H. What do you see?

a)

Color change

b)

Precipitate formation

c)

Energy change

d)

Gas formation

42.

Balance __NO2 --> __N2 + __O2

a)

1, 1, 1

b)

2, 1, 1

c)

1, 2, 1

d)

2, 1, 2

43.

Reactions that have hydrocarbons (CH4) and oxygen as reactants and carbon dioxide and water as products

a)

Conservation of Mass

b)

combustion

c)

double replacement

d)

decomposition

44.

A neutralization is a special type of _______ where a salt and water are produced.

a)

decomposition

b)

synthesis

c)

single replacement

d)

double replacement

45.

Burning something does not necessarily mean combustion. When you placed Mg in the flame it became bright white _____ and formed gray ash ____.

a)

Absorbing light; MgO

b)

Emitting light; MgO

c)

Absorbing light; Mg

d)

Emitting light; O

e)

Emitting light; Mg

46.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar; arrow towards H

c)

ionic

d)

polar; arrow towards Cl

47.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar; arrow towards Li

c)

ionic

d)

polar; arrow towards O

48.

When you have F-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

49.

The electrons in a polar covalent molecule are ...

a)

shared equally

b)

shared unequally

c)

transferred

d)

None of the Above

50.

In a polar bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

51.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

52.

Why does hexane not dissolve in water?

a)

Hexane is polar and water is nonpolar.

b)

Hexane is nonpolar and water is nonpolar.

c)

Hexane is polar and water is polar.

d)

Hexane is nonpolar and water is polar.

53.

Which of the following liquids would NOT mix with water?

a)

Vegetable oil

b)

Food coloring

c)

Maple syrup

d)

Vinegar

54.

The ___________ of the soap molecule attracts water while its _______ is attracted to fat and grease.

a)

head; tail

b)

tail; head

c)

center; outside

d)

outside; center

55.

Methane, CH4, is a gas at room temperature while Octane, C8H18, is a liquid because ________

a)

Methane has more polarity.

b)

Octane has more polarity

c)

Octane has more dispersion.

d)

Methane has more dispersion.

56.

Why do water molecules attract one another?

a)

Because of the slightly positive regions and slightly negative regions

b)

Due to the positive regions attracting other positive regions

c)

Due to the negative regions attracting other negative regions

d)

None of the above

57.

What electronegativity trend is shown in this periodic table?

a)

Electronegativity increases as you go up and to the left.

b)

Electronegativity increases as you go down and to the left.

c)

Electronegativity increases as you go up and to the right.

d)

Electronegativity increases as you go down and to the right.

58.

How does this picture demonstrate the sharing of electrons?

a)

two weak atoms sharing equally

b)

two weak atoms sharing unequally

c)

two strong atoms sharing equally

d)

two strong atoms sharing unequally

e)

one strong atom and one weak atom sharing unequally

59.

Soap is "soap" because it attracts ________.

a)

both polar and nonpolar substances

b)

only polar substances

c)

only nonpolar substances

d)

no substances

60.

This molecule has _______ bonds and is considered ________.

a)

polar; polar

b)

nonpolar; polar

c)

polar; nonpolar

d)

nonpolar; nonpolar

61.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonding

62.
A molecule containing polar covalent bonds is always polar.
a)
True
b)

False; only if asymmetric

c)

False; only if symmetric

63.

How does soap affect the surface tension of water?

a)

Soap increases surface tension, so more soapy drops fit on the penny than drops of regular tap water.

b)

Soap decreases surface tension, so more soapy drops fit on the penny than drops of regular tap water.

c)

Soap increases surface tension, so fewer soapy drops fit on the penny than drops of regular tap water.

d)

Soap decreases surface tension, so fewer soapy drops fit on the penny than drops of regular tap water.

64.

Which of the following elements does NOT obey the octet rule?

a)

Nitrogen

b)

Oxygen

c)

Potassium

d)

Hydrogen

65.

Explain why water is attracted to a negatively charged balloon.

a)

Positive O's attract to the balloon.

b)

Positive H's repel the balloon

c)

Negative O's repel the balloon

d)

Positive H's attract to the balloon

66.

A type of chemical that forms solutions that taste sour, due to high concentrations of positive hydrogen ions

a)

acid

b)

base

c)

salt

d)

pH

67.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
68.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

vinegar

b)

milk

c)

water

d)

bleach

69.

Four substances were tested for pH, lemon juice (pH 2), baking soda (pH 9), bleach (pH 12), and milk (pH 6). Which of the following correctly lists the substances from most basic to acidic?

a)

lemon juice, milk, baking soda, bleach

b)

bleach, baking soda, milk, lemon juice

c)

milk, lemon juice, baking soda, bleach

d)

baking soda, bleach, lemon juice, milk

70.

At what pH would all three indicators appear as yellow?

a)

1.7

b)

2.7

c)

4.7

d)

8.7

71.

If a solution has a pH of 1.5, then litmus would turn

a)

red

b)

purple

c)

blue

d)

yellow

72.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
73.
What are the coefficient used to balance the equation below?
__Ag2O →__ Ag +___O2
a)
2,4,1
b)
1,1,1
c)
2,1,2
d)
2,2,2
74.

Balance this equation

__Al +__HCl -->__H2 +__AlCl3

a)

2, 6, 3, 2

b)

it is already balanced

c)

4, 12, 3, 4

d)

2, 1, 4, 5

75.

What does the Law of Conservation of Mass state?

a)

Matter is created and destroyed in a chemical reaction.

b)

Matter is neither created nor destroyed, just transferred.

c)

Matter is only destroyed in a chemical reaction.

d)

Matter can be transformed into energy.

76.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)

SO2

c)

SO3

d)

SO4

e)

S2O

77.
What is the empirical formula for the following:
Pb5Cr5O20
a)
Pb2Cr2O10
b)
PbCr2O7
c)
Pb9Cr4O2
d)
PbCrO4
78.

In a chemistry class, Avery, Oliver, and Sophia were given different pairs of compounds and asked to identify which pair has the same empirical formula. Can you help them find the correct pair?

a)

NaCrO4 and Na2Cr2O7

b)

C2H4O2 and C6H12O6

c)

C3H6O3 and C2H6O2

d)

CH4 and C2H6

79.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
80.

Matching and pairing your socks ______________

a)

Increases entropy

b)

Decreases entropy

c)

Increases enthalpy

d)

Decreases enthalpy

e)

changes nothing.

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