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AP Chemistry Spontaneity

Total questions: 84

Worksheet time: 2hrs 34mins

Name
Class
Date
1.
Temperature is a measure of average [blank] energy of individual atoms.
a)
heat
b)
potential
c)
mechanical
d)
kinetic
2.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
3.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
4.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
5.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
6.
 _?_  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
7.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
8.

How do you calculate enthalpy change of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

9.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
10.
Heat is measured in 
a)
joules
b)
grams
c)
degrees celcius
11.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
12.

What does the circle mean in ΔH°?

a)

Standard Conditions (T=298.15 K P=1 atm)

b)

Standard Temperature and Pressure (T=273.15 K P=1 atm)

c)

Degree K

d)

Degree C

13.

A reaction that causes the temperature of the surroundings to drop is

a)

endothermic

b)

exothermic

c)

displacement

d)

oxidation

14.

The enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions. This is the enthalpy of.....

a)

Combustion

b)

Formation

c)

Lattice breaking

d)

Ionisation

15.
Same amount of heat is given to 3 substance. Which shows a smallest increase in temperature?
a)
gold
b)
silver 
c)
water
16.
In an exothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released
17.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
18.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
19.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
20.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
21.
HCl reacts with Zn giving off heat
a)
endothermic
b)
exothermic
22.

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

23.

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


Gas --> Liquid --> solid

a)

increase

b)

decrease

24.

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

25.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

26.

What phase of matter has the most entropy?

a)

solid

b)

liquid

c)

gas

27.

What is the symbol for entropy?

a)

H

b)

G

c)

S

d)

E

28.

Which represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

29.

Which represents a negative ΔS?

a)

ice melting

b)

salt dissolving

c)

water heating up

d)

none of these

30.

Which of the following scenarios describes a process with a negative entropy change?

a)

Building a skyscraper

b)

A clean room becomes cluttered

c)

An igloo melting

d)

Osmosis (I hope you know your Biology!)

31.

Which of these have a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

2NO2(g) → N2O4(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

32.

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

33.

Ammonium nitrate dissolves in water. It is a spontaneous endothermic process because the system undergoes....

a)

a decrease in enthalpy

b)

an increase in entropy

c)

an increase in enthalpy

d)

a decrease in entropy

34.

Which has a +ΔS (system)?

a)

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

b)

H2O(g) + CO2(g) → H2CO3(aq)

c)

H2(g) + I2(g) → 2Hl(g)

d)

C2H2O2(g) → 2CO(g) + H2(g)

35.

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

36.

Which sample has the lowest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

37.
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.
38.

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

39.

A reaction that releases energy is

a)

Exothermic

b)

Endothermic

c)

Could be either

40.

A reaction that absorbs energy is

a)

Exothermic

b)

Endothermic

c)

Could be either

41.
Spontaneity is determined by....
a)
enthalpy only
b)
entropy only
c)
enthalpy and entropy
d)
enthalpy, entropy, and temperature
42.
Spontaneous reactions may be extremely slow.
a)
True
b)
False
43.
Reactions tend to be spontaneous if they are exothermic.
a)
True
b)
False
44.

A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if ΔH is __________ and ΔS is __________.

a)

+, +

b)

-, -

c)

+, -

d)

-, +

45.

ΔS will be positive for the reaction

a)

2H2 (g) + O2 (g) -> 2H2O (g)

b)

2NO2 (g) -> N2O4 (g)

c)

BaF2 (s) ->Ba2+ (aq) + 2F- (aq)

d)

2Hg (l) + O2 (g) ->2HgO (s)

46.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
47.
For the following reaction indicate if entropy is increased or decreased.    2N2(g)  +  3 H2(g)  ------->  2 NH3(g)
a)
increase
b)
decrease
48.
For the following reaction indicate if entropy is increased or decreased.     KClO3(s)  ------>  KCl(s)  +  O2(g) 
a)
increase
b)
decrease
49.
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
50.

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

51.

dissolving sugar ________

a)

decreases the entropy

b)

increases the entropy

52.

When ammonium nitrate dissolves in water, the solution gets cold. Which is true?

a)

Reaction is ENDOTHERMIC with positive ΔS

b)

Reaction is ENDOTHERMIC with -ΔH

c)

Reaction is EXOTHERMIC with a -ΔH

d)

Reaction is EXOTHERMIC with +ΔS

53.

The measure of disorder in a system is

a)

entropy

b)

enthalpy

c)

exothermic

d)

endothermic

54.

I2(s) + energy → I2(g)

As I2(s) sublimes to I2(g), the entropy

a)

increases: particles are less randomly arranged

b)

increases: particles are more randomly arranged

c)

decreases: particles are less randomly arranged

d)

decreases: particles are more randomly arranged

55.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
56.

As NaCl dissolves according to the equation

NaCl(s) → Na+(aq) + Cl-(aq), the entropy of the system

a)

Increases

b)

Decreases

c)

Remains the same

57.

Which of the following produces a decrease in the entropy of the system?

a)

dissolving solid KCl

b)

mixing 2 gases into one container

c)

melting ice to make water

d)

freezing water to form ice

58.

Which of the following would have the highest entropy?

a)

A cold solid

b)

A hot liquid

c)

A hot gas

d)

A cold gas

59.
Entropy is a measure of the number of possible ways that the energy of a system can be distributed. 
a)
true
b)
false
60.
Temperature is a measure of average [blank] energy of individual atoms.
a)
heat
b)
potential
c)
mechanical
d)
kinetic
61.
The equation that relates enthalpy, temperature and entropy is
a)
Hess's Law
b)
Second Law of Thermodynamics
c)
Gibbs Free Energy
d)
Calorimetry
62.

True/False: The rate of a chemical reaction is related to the spontaneity of the reaction.

a)

True

b)

False

63.
 For which of these processes is the value of ΔH expected to be positive?
1.  The temperature increases when calcium chloride dissolves in water.
 2.  Steam condenses to liquid water
3.  Water boils
4.  Dry ice sublimates
a)
4 only
b)
1 only
c)
3 and 4 only
d)
2 and 3 only
64.

Which reaction has the greatest increase in entropy?

a)

2H20 (l) --> 2H2 (g) + O2 (g)

b)

2H2O(g)--> 2H2(g) + O2(g)

c)

H2O(g) --> H2O(l)

d)

H2O(l) H2O(s)

65.

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


SUBLIMATION

a)

increase

b)

decrease

66.

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


Vaporization

a)

increase

b)

decrease

67.

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

68.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
69.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
70.
Is this reaction endothermic or exothermic?
a)
endothermic 
b)
exothermic
71.
What is the ΔH of this reaction?
a)
40 kJ
b)
20 kJ
c)
80 kJ
d)
60 kJ
72.
What is the energy of the activated complex?
a)
75 kJ
b)
225 kJ
c)
300 kJ
d)
225 kJ
73.
What is the activation energy of the reverse reaction?
a)
75 kJ
b)
300 kJ
c)
150 kJ
d)
225 kJ
74.
How much potential energy do the products of the reverse reaction have?
a)
225 kJ
b)
300 kJ
c)
75 kJ
d)
250 kJ
75.
What letter represents ΔH?
a)
A
b)
B
c)
C
d)
D
76.

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

77.
Spontaneous reactions may be extremely slow.
a)
True
b)
False
78.

1. Given the following information, calculate ΔG0 for the reaction below at 250C: (K = 0C + 273)

SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),

ΔH0=133.0 kJ and ΔS0 =401.5 J/K

a)

-252.6 kJ

b)

-13.4 kJ

c)

13.4 kJ

d)

252.6 kJ

79.
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 
80.

If a process is exothermic and not spontaneous, then what must be true?

a)

ΔS > 0

b)

ΔH > 0

c)

ΔG = 0

d)

ΔS < 0

81.

If ΔH and ΔS are both negative or positive, then ΔG has a -------------------sign.

a)

Positive

b)

Negative

c)

Large

d)

Variable

82.

1. Calculate the standard entropy change for the following reaction: Cu(s)+1/2 O2(g) → CuO(s). Given that

S0 (Cu(s)) = 33.15 J/K*mol

S0 (O2(g)) = 205.14 J/K*mol

S0 (CuO(s)) = 42.5 J/K*mol

a)

195.66 J/K.mol

b)

93.09 J/K.mol

c)

-93.09 J/K.mol

d)

+195.66 J/K.mol

83.

1. Given the following information, calculate ΔG0 for the reaction below at 250C:

SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),

ΔH0=133.0 kJ and ΔS0 =401.5 J/K

a)

-252.6 kJ

b)

-13.4 kJ

c)

13.4 kJ

d)

252.6 kJ

84.

Mr. Murphy is the best Chemistry teacher you have ever had (so far)

a)

Yes!

b)

Yes?

c)

Yes.

d)

Decline to say

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