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Specific Heat/Enthalpy Review

Total questions: 71

Worksheet time: 12hrs 50mins

Name
Class
Date
1.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
2.
Endothermic reactions feel
a)
warm
b)
cold
3.

A reaction that gives out energy to the surroundings causes the surroundings ....

a)

temperature to drop

b)

temperature to rise

c)

temperature to remain constant

d)

temperature to vary

4.

In the reaction picture, the energy will be on product or reactant

a)

Product

b)

Reactant

5.
Temperature is a measure of average [blank] energy of individual atoms.
a)
heat
b)
potential
c)
mechanical
d)
kinetic
6.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
7.
 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
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.
H2 + ½ O2 --> H2O + 285kJ is an example of a(n)
a)
Electrical equation
b)
Heat equation
c)
Thermochemical equation
12.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is 0.900J/goC
a)
450
b)
-450
c)
225
d)
-225
13.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
14.
How much heat is needed to form 40.0 L of NO2 from its elements at STP? , Vm=22.4L
N2+ 2O2 -> 2NO2
ΔH = +67kJ
a)
58.2 kJ
b)
29.1
c)
59.8
d)
119.6
15.

Define the term Exothermic by picking the correct statements

a)

Products have less energy than the reactants

b)

ΔH is negative

c)

ΔH is positive

d)

Energy is given out to the surroundings (temperature goes up).

e)

products have more energy than the reactants

16.

Define Endothermic by picking the correct statements

a)

ΔH is positive

b)

Energy is taken in from the surroundings (temperature goes down).

c)

Energy is given out to the surroundings (temperature goes up).

d)

· Products have less energy than the reactants

e)

products have more energy than the reactants

17.

ΔHrxn

a)

symbol for enthalpy of reaction

b)

symbol for enthalpy

c)

exothermic reaction

d)

difference in altitude

18.

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

a)

12.82 °C

b)

24.12°C

c)

351 °C

19.

Using the equations below:


C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ


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


MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

20.

Which of the following statements are true for the reaction:


SO2(g) + 1/2O2(g) ↔ SO3(g) ΔH = –92 kJ mol-1


Where ↔ indicates that the reaction can proceed in the forward and the reverse direction. (PICK 2)

a)

The forward and reverse reaction both produce 92 kJ of energy.

b)

Oxidising 2 moles of SO2 would produce twice as much energy.

c)

The reverse reaction has an enthalpy of +92 kJ mol-1.

d)

Surrounding becomes colder by time.

21.
Bond making and bond breaking. Which of following is TRUE?
a)
During bond breaking, heat is absorbed
b)
During bond making, heat is absorbed
c)
During bond breaking, heat is released
d)
None of the above
22.

Which science involves measuring the amount of heat released or absorbed during a chemical reaction?

a)

stoichiometry

b)

calorimetry

c)

photolithography

d)

metrology

23.

What type of chemical reaction releases energy through light or heat?

a)

an endothermic reaction

b)

an exothermic reaction

c)

an isothermic reaction

d)

an isobaric reaction

24.
Temperature is a measure of average [blank] energy of individual atoms.
a)
heat
b)
potential
c)
mechanical
d)
kinetic
25.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

26.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

27.

When new chemical bonds form, energy ____________.

a)

is taken into the system.

b)

is released from the system.

c)

stays the same in the system.

28.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

29.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

30.

Using the equations below:

C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ

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

MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

31.

Using the equations below

Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ

2Cu(s) + 1/2O2(g) → Cu2O(s) ∆H = –170 kJ

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

2CuO(s) → Cu2O(s) + 1/2O2(g)

a)

142

b)

15

c)

-15

d)

-142

32.

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

33.

The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1

What is the enthalpy change, in kJ mol–1, for the reaction below?

P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

34.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
c)
Sometimes
35.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
c)
nothing happens
d)
it gets colder
36.

A chemical reaction that requires energy is a(n)

a)
exothermic reaction 
b)
endothermic reaction 
c)
over reaction 
d)
redox reaction
37.

If N2 (g) + 2O2 (g) ⟶\longrightarrow   2NO2(g) has a ΔHrxn \Delta H_{rxn\ }  = 68, then what is the ΔHrxn\Delta H_{rxn}  if you reverse the reaction?

a)

86 kJ

b)

- 86 kJ

c)

68 kJ

d)

-68 kJ

38.

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

39.
(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 
40.
Solid magnesium dissolves in a hydrochloric acid, releasing hydrogen gas and heat from a solution of magnesium chloride. What is the sign on ΔH for this reaction?
a)
Negative because it is exothermic
b)
Negative because it is endothermic
c)
Positive because it is exothermic
d)
Positive because it is endothermic
41.

Which will heat up faster?

a)

copper

b)

granite

c)

iron

d)

basalt

42.

Which will heat up slower?

a)

water

b)

lead

c)

granite

d)

iron

43.
If I heat up 2 pans of water one has 100 mL in it and one has 1000mL. Which one heats up the fastest?
a)
100 mL
b)
1000 mL
c)
They both heat up at the same speed
d)
They cool down.
44.

Which of the following best explains why the sand at the beach is hotter than the water?

a)

Sand has a higher specific heat than water.

b)

Sand has a lower specific heat than water.

c)

There is more water than sand at the beach.

d)

There is more sand than water at the beach.

45.

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

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

46.
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
47.
Specific heat of water is  4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more heat energy to raise the temperature?
a)
Water
b)
Wood
c)
Both are same
48.

What letter is used to represent specific heat capacity?

a)

H

b)

P

c)

C

d)

T

49.
Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?
a)
Copper
b)
Carbon Steel
c)
Zinc
d)
Stainless Steel
50.
What is the measurement of the average kinetic energy of a substance?
a)
Kinetic energy
b)
Temperature
c)
Thermal energy
d)
Potential energy
51.
If an object has particles that are moving very quickly, the object 's temperature is probably _____.
a)
cold
b)
slow
c)
big
d)
hot
52.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
53.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

54.

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

a)

418 J

b)

209 J

c)

83 J

d)

4.18 J

55.

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)

1.95 °C

d)

5128 °C

56.

In heat capacity equations, what does the delta sign (the one which looks like triangle) represent?

a)

Temperature

b)

energy

c)

mass

d)

change in

e)

change in temp

57.

the addition of 485 J of energy increases the temperature of a 47.3 g sample of a metal from 25.6oC to 45.3oC. What is the specific heat capacity of this metal?

a)

.226 J/g*oC

b)

.520 J/g*oC

c)

.401 J/g*oC

d)

.385 J/g*oC

58.

the energy required to change phase from solid to liquid

a)

heat of vaporization

b)

heat of fusion

59.

the energy required to change phase from liquid to gas

a)

heat of vaporization

b)

heat of fusion

60.

Temperature does NOT change during a phase change.

a)

True

b)

False

61.

The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide.

C(s) +O2(g) → CO2(g) ΔH = –x kJ mol–1

CO(g) + O2(g) → CO2(g) ΔH = –y kJ mol–1

What is the enthalpy change, in kJ mol–1, for the oxidation of carbon to carbon monoxide?

C(s) + O2(g) → CO(g)

a)

x + y

b)

-x - y

c)

y - x

d)

x - y

62.

The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1

What is the enthalpy change, in kJ mol–1, for the reaction below?

P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

63.

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
64.

If N2 (g) + 2O2 (g) ⟶\longrightarrow   2NO2(g) has a ΔHrxn \Delta H_{rxn\ }  = 68, then what is the ΔHrxn\Delta H_{rxn}  if you reverse the reaction?

a)

86 kJ

b)

- 86 kJ

c)

68 kJ

d)

-68 kJ

65.
(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 
66.

What is standard enthalpy of formation, ΔHfo?

a)

Heat change when 1 mole of gaseous ions is hydrated in water at 25oC and 1 atm

b)

Heat change when 1 mole of compound is formed from its elements in their standard states at 25oC and 1 atm

c)

Heat change when 1 mole of gaseous atom is formed from its elements at 25oC and 1 atm

d)

Heat change when 1 mole of electrons is removed from 1 mole of gaseous atoms at ground state at 25oC and 1 atm

67.

Which of the following has a ΔHfo value of 0?

a)

Br2(g)

b)

N(g)

c)

CO(g)

d)

Ne(g)

68.

which of the following represent the lattice enthalpy of formation of sodium flouride

a)

2Na(g) + F2(g) → 2NaF(g)

b)

Na(s) + 1/2F2(g) → NaF(s)

c)

2Na(s) + 1/2F2(g) → NaF(g)

d)

2Na(s) + F2(g) → 2NaF(g)

69.

Use the Hf values in the table below to answer questions a and b about the following reaction.

CO2(g) + N2(g) ⟶ NO(g) + CO(g) ΔH = ?


Formula kJ/mol


CO(g) -110


CO2(g) -394


NO(g) 90


a) Calculate Hrxn for the reaction.

a)

370kJ/mol

b)

374kJ/mol

c)

333kJ/mol

d)

335KJ/mol

70.

Select the reaction that is a correct formation reaction for NaCl .

a)

Na (s) + Cl (s) --> NaCl (s)

b)

2Na (s) + Cl2 (g) --> 2 NaCl (s)

c)

Na (s) + 1/2 Cl2 (g) --> NaCl (s)

d)

Na (g) + Cl2 (g) --> NaCl (s)

71.

What is the specific heat capacity (in J/g°C) of a substance if 250 grams of it absorbs 5,000 Joules of heat, causing its temperature to increase by 20°C?

a)

1.0 J/g°C

b)

0.5 J/g°C

c)

1.5 J/g°C

d)

2.0 J/g°C

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