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Chemistry II Unit 8 Review

Total questions: 74

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

Energy can never be created nor destroyed. Which law does this refer to?

a)

0th law of thermodynamics

b)

1st law of thermodynamics

c)

2nd law of thermodynamics

d)

3rd law of thermodynamics

2.

While running your kinetic energy converts to thermal energy. Which law does this refer to?

a)

0th law of thermodynamics

b)

1st law of thermodynamics

c)

2nd law of thermodynamics

d)

3rd law of thermodynamics

3.

The entropy of the universe is always increasing. Which law does this refer to?

a)

0th law of thermodynamics

b)

1st law of thermodynamics

c)

2nd law of thermodynamics

d)

3rd law of thermodynamics

4.

Disorder is more likely than order. Everything trends towards randomness and chaos. Which law does this refer to?

a)

0th law of thermodynamics

b)

1st law of thermodynamics

c)

2nd law of thermodynamics

d)

3rd law of thermodynamics

5.

From lowest entropy to highest entropy, the states of matter go in this order:

a)

solid -> liquid -> gas -> plasma

b)

plasma -> gas -> liquid -> solid

c)

gas -> plasma -> liquid -> solid

d)

solid -> liquid -> plasma -> gas

e)

It depends on the temperature of the object

6.

True or False: Entropy increases as temperature increases

a)

True

b)

False

7.

True or False: A flowing stream has less entropy than a calm lake.

a)

True

b)

False

8.
 _?_  is the amount of energy required to raise the temperature of 1 gram of any substance 1oC.
a)
Specific heat
b)
A calorie
c)
Thermal energy
d)
Conduction
9.
As 120 g of hot milk cools in a mug, it transfers 20, 000 J of heat to the environment. What is the temperature change of the milk? The specific heat of milk is 2.6 J/g·°C. (Q=mcΔT)
a)
64 °C
b)
1.56 °C
c)
640 °C
d)
cannot be determined
10.
If 100 g of aluminum at 145ºC gains 6,800 J of heat, what is the final temperature (Tfinal) of the aluminum? Aluminum has a specific heat of 0.897 J/gºC. (Q=mcΔT)
a)
-69°C
b)
0.52°C
c)
221°C
11.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
12.

Heat transfer _____ occurs from hot to cold.

a)

always

b)

never

c)

sometimes

d)

rarely

13.

Temperature is a measure of average _____ energy of individual atoms.

a)

heat

b)

potential

c)

mechanical

d)

kinetic

14.
If 25 J are required to change the temperature of 5.0 g of substance A by 2.0°C, what is the specific heat of substance A? 
a)
250 J/g C
b)
10 J/g C
c)
63 J/g C
d)
2.5 J/g C
15.

If a chemical reaction is EXOTHERMIC, the temperature of the surroundings would....

a)

Stay the same

b)

Increase

c)

Decrease

16.
When iron nails get rusty, heat is released.  What process is this?
a)
Exothermic
b)
Endothermic
17.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
18.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
19.
Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?
a)
It is an exothermic reaction
b)
It is an endothermic reaction
c)
It is made of ice
d)
It is dissolving your mouth
20.
What happens to particles as they heat up?
a)
They slow down
b)
Nothing
c)
They don't move
d)
They speed up
21.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
22.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
23.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

24.

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water. The water weighs 75. g and had an initial temperature of 20.00 °C? (Specific heat of water is 4.18 J/g°C)

a)

0.111 J/g°C

b)

1.29 J/g°C

c)

0.129 J/g°C

d)

22225.85 J

25.

A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

26.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
27.

Study the reaction below. Is it exothermic or endothermic?

H2 + Cl2 --> 2 HCl + 1845 kJ

a)

Exothermic Reaction

b)

Endothermic Reaction

28.

How do you calculate the Enthalpy of Reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔG = ΔH -TΔS

c)

ΔT = q / mC

d)

E = mc2

29.

ΔH value in an endothermic reaction is negative.

a)

True

b)

False

30.

According to the Particles Theory of Matter, one particle has the ability to vibrate within their mean position if added with heat. Which of the following is the statement referring to?

a)

Solid

b)

Liquid

c)

Gas

31.

It is the study of energy, its different forms, and patterns of change.

a)

Thermochemistry

b)

Enthalpies

c)

Thermochemical equation

d)

Thermodynamics

32.

A balanced equation showing the associated enthalpy change.

a)

Thermochemistry

b)

Enthalpy

c)

Thermochemical equation

d)

Thermodynamics

33.

What does Hess's Law state?

a)

Both answers

b)

Reaction can be the sum of 3+ reactions, then heat flow for overall reaction is less than the sum of heat flows

c)

Reaction can be the sum of 2+ reactions, then heat flow for overall reaction equals the sum of heat flows

d)

Neither answer

34.

Which has higher entropy?

A. A small pool of water sits in an enclosed glass chamber.

B. An enclosed glass chamber is filled with water vapor.

a)

A

b)

B

35.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
36.

Which of the following correctly describes the entropy changes of the water molecules and the universe when a sample of water freezes?

a)

A

b)

B

c)

C

d)

D

37.
Which statement is true about the ENTROPY?
a)
Entropy refers to DISORDER, the unusable energy that escapes a system.
b)
Entropy refers to the balance of temperature among two or more systems.
c)
Entropy refers to the average kinetic energy of the molecules.
d)
Entropy refers to the inability to destroy or create energy. 
38.
Which state of H2O  has the greatest entropy?
a)
Ice
b)
Water
c)
Vapor
39.
As a system becomes more disordered, entropy
a)
remains the same
b)
increases
c)
decreases
d)
cannot be determined
40.

A small S value indicates the system has _______

a)

more order

b)

more randomness

41.

Given the change of phase:

CO2(g) —> CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

42.

Identify whether the following result in an increase or decrease in entropy:


3 moles of gas (on reactant side) --> 6 moles of gas (product)

a)

increase

b)

decrease

43.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

44.
The first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and
a)
mass
b)
work done
c)
force
d)
pressure
45.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
46.

Your enthalpy is +20 and your entropy is +5. Which temperature will give a spontaneous reaction?

a)

0

b)

4

c)

8

47.

Your enthalpy is high and negative but your entropy is also negative. What type of temperature would you want to get a spontaneous reaction?

a)

low

b)

high

48.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

49.

At what temperature would a given reaction become spontaneous if ΔH =+119kJ and ΔS=+263J/K.mol

a)

455 K

b)

-2210 K

c)

382 K

d)

-363 K

50.
True/False: The rate of a chemical reaction is unrelated to the spontaneity of the reaction.
a)
True
b)
False
51.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

52.

enthalpy is driving force when

a)

exothermic

b)

endothermic

c)

increase in entropy

d)

decrease in entropy

53.

If a reaction occurs, then delta G is

a)

negative

b)

positive

c)

can't tell

d)

0

54.

What is the definition of solubility?

a)
The ability of a substance to dissolve in another substance
b)
The ability of a substance to react with another substance
c)
The ability of a substance to change its state from solid to liquid
d)
The ability of a substance to change its color when heated
55.

What is a solute?

a)

A type of musical instrument

b)

A substance that is dissolved in a solution

c)
A mathematical solution
d)
A type of physical exercise
56.

What is a solvent?

a)

A substance that reacts with a solute

b)
A substance that cannot be dissolved
c)

A substance that it dissolves in usually water

d)
A substance that is insoluble in water
57.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
58.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
59.
When 42 grams of potassium chloride, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
60.

How many grams of KClO3, are soluble in 200g of water at 30ºC?

a)

5 grams

b)

100 grams

c)

10 grams

d)

20 grams

61.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
62.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
63.

The correct mathematical expression for finding the molar solubility (X) of Sn(OH)2 is:

a)

2(X)3 = Ksp

b)

108(X)5 = Ksp

c)

4(X)3 = Ksp

d)

8(X)3 = Ksp

64.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
65.

In a redox reaction, the species that is reduced will ___ electrons, becoming more _____ charged.

a)

lose; negatively

b)

lose; positively

c)

gain; positively

d)

gain; negatively

66.

A precipitation reaction must...

a)

Have a solid ionic product from aqueous reactants

b)

Have only gaseous products from gaseous reactants

c)

Have only aqueous products from aqueous reactants

67.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

68.

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.

69.

Which sample has the lowest entropy?

HINT - Look at the phase of each chemical....

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

70.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

71.

What is the symbol for entropy?

a)

H

b)

G

c)

S

d)

E

72.

Which of these reactions shows a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

3O2(g) → 2O3(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

73.

Free energy is represented by the letter

a)

F

b)

E

c)

G

d)

S

74.
Spontaneous reactions may be extremely slow.
a)
True
b)
False

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