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Unit 9 Review: Thermodynamics

Total questions: 56

Worksheet time: 1hrs 14mins

Name
Class
Date
1.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
2.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
3.
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
4.

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

5.

Entropy is a measure of

a)

accuracy

b)

precision

c)

the disorder of a system

d)

the attraction of a nucleus for an electron

6.

What phase of matter has the most entropy?

a)

solid

b)

liquid

c)

gas

7.

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

8.

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)

9.

Which reaction has a +ΔS ?

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)

10.

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.

11.
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.
12.

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

a)

0

b)

4

c)

8

13.

Your enthalpy is -20J and your entropy is -8J. Which temperature will give you a spontaneous reaction?

a)

1

b)

3

c)

5

14.

Which of the following situations demonstrates high entropy?

a)

water freezing

b)

water vaporizing

c)

steam condensing to water

15.

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

16.

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.

17.

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

18.

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

19.

Which reaction has the greatest increase in entropy of the system?

A. HCl (g) + NH3 (g) → NH4Cl (s)

B. (NH4)2Cr2O7 (s) → Cr2O3 (s) + N2 (g) + 4H2O (g)

C. CaCO3 (s) → CaO (s) + CO2 (g)

D. I2 (g) → I2 (s)

a)

A

b)

B

c)

C

d)

D

20.

Choose the correct correlation between Gibbs free energy and feasibility.

a)

a reaction to be feasible, ΔG has to be negative.

b)

a reaction to be feasible, ΔG has to be positive.

c)

a reaction to be feasible, ΔG has to be zero

d)

no correlation between ΔG and feasibility

21.

Which of the reactions below has a negative ∆S?

a)

CuCO3 (s) + 2HCl (aq) → CuCl2 (aq) + CO2 (g) + H2O (l)

b)

C (s) + O2 (g) → CO2 (g)

c)

CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)

d)

BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaCl (aq)

22.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
23.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
24.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
25.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

26.
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
27.

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

28.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (ignore sig figs)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

29.

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) (ignore sig figs)

a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
30.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

31.
In an exothermic process, the surroundings are gaining energy.
a)
True
b)
False
32.

What symbol represents Enthalpy change?

a)

ΔH

b)

ΔT

c)

ΔG

d)

ΔS

33.

How do you calculate Change in Enthalpy?

a)

ΔH = q / n

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

34.

Organic chemistry is difficult. Those who study it have __________ of trouble.

a)

all kinds

b)

alkynes

c)

alkanes

d)

alkenes

35.

2 S + 3 O2 --> 2 SO3 + 791.4 kJ


How much heat will be released if 96 grams of O2 (32g/mol) were reacted?

a)

1055.2 kJ

b)

791.4 kJ

c)

1582.8 kJ

36.
How much heat is absorbed if
4.0 mole A reacts?
A + 2B + 22.0 kJ → 3C  
a)
22.0 kJ
b)
44.0 kJ
c)
66.0 kJ
d)
88.0 kJ
37.

How much energy does it take to heat 60g of ice at -20C to a temperature of 75C?

a)

-19980 J

b)

2460 J

c)

19980 J

d)

41250 J

38.

How much energy would it take to melt 75g of ice?

a)

-3135

b)

3135 J

c)

24975 J

d)

169500 J

39.

When the ice is heated, the temperature _______ until the temperature becomes _________ . The temperature at which this occurs is called the ________ point.

(a)  

40.

Determine the amount of heat energy required to convert 10 grams of ice at -20 °C to steam at 125 °C.

a)

31012 J

b)

30292 J

c)

33938 J

d)

32293 J

41.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

42.

How can you find the change in temperature?

a)


Tfinal + TinitalT_{final}\ +\ T_{inital}

b)

Tfinal − TinitialT_{final}\ -\ T_{initial}

c)

none of the above

43.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

44.

In the following reaction, 2A + 2B --> C, ΔH=−60 kJ\Delta H=-60\ kJ  . What is the ΔH\Delta H  when 6 moles of A are reacted?

a)

-180 kJ

b)

-360 kJ

c)

180 kJ

d)

360 kJ

45.

Which process is accompanied by a decrease in entropy?

a)

boiling of water

b)

condensing of water vapor

c)

subliming of iodine

d)

melting of ice

46.

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

47.

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)

48.
The equation that relates enthalpy, temperature and entropy is
a)
Hess's Law
b)
Second Law of Thermodynamics
c)
Gibbs Free Energy
d)
Calorimetry
49.
 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
50.
What signs of Δ H  and Δ S  will always yield a reaction that is spontaneous ? 
a)
Δ H  =  +   Δ S  =  +
b)
Δ H  =  -   Δ S  =  - 
c)
Δ H  =  -   Δ S  =  +
d)
Δ H  =  +  Δ S  =  --
51.

Predict the entropy change, ΔS.

a)

ΔS = +

b)

ΔS = -

c)

ΔS = 0

d)

ΔS = no change

52.
When ammonium nitrate dissolves in water, the solution gets cold. Which is true?
a)
Reaction is ENDOTHERMIC with positive ΔH
b)
Reaction is ENDOTHERMIC with -ΔH
c)
Reaction is EXOTHERMIC with a -ΔH
d)
Reaction is EXOTHERMIC with +ΔH
53.

For the reaction C2H6 (g) ->C2H4 (g) + H2 (g) ΔHο is +137 kJ/mol and ΔSοis +120 J/K.mol. This reaction is

a)

nonspontaneous at all temperatures

b)

unreliable

c)

spontaneous only at high temperature

d)

spontaneous at all temperatures

e)

spontaneous only at low temperature

54.

Which of the following would most likely lead to a spontaneous reaction.

a)

A high negative enthalpy.

b)

A low negative enthalpy.

c)

A high positive enthalpy.

d)

A low positive enthalpy.

55.

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.

56.

a)

A

b)

B

c)

C

d)

D

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