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Accel Chem PC #9 Thermochemistry

Total questions: 48

Worksheet time: 2hrs 45mins

Name
Class
Date
1.
The specific heat of aluminum is 0.21 J/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
d)
0.105 J
2.
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)
400 J
b)
210 J
c)
80 J
d)
4.18 J
3.
For an endothermic reaction, the heat is on the ____ side.
a)
reactant
b)
product
c)
either side
4.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
5.
For an exothermic reaction, the heat is on the ____ side
a)
reactant
b)
product
c)
either side
6.
What type of reaction is shown in the picture?
a)
endothermic
b)
exothermic
7.
In an exothermic process, the surroundings are are gaining energy.
a)
True
b)
False
8.
If two objects have different temperatures, 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
9.

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
10.

4180 j of heat energy are added to change the temperature of water by 10oC. How many grams of water are being heated? cwater=4.18 j/g*C

a)

4.18 j/g*C

b)

10000g

c)

174724g

d)

100g

11.

What heat energy is required to raise the temperature of a 1g sample of mercury (cHg=.16 j/g*C) by 100oC?

a)

16j

b)

.0016j

c)

16000j

d)

625 j

12.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

13.

What does q stand for?

a)

Heat (Joules)

b)

Mass (Grams)

c)

Specific Heat (J/g*C)

d)

Temperature Change (*C)

14.

What does m stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

15.

When two samples of similar mass are subjected to the same heat energy, the sample with the SMALLER specific heat will have a _________ temperature change.

a)

SMALLER

b)

LARGER

c)

EQUAL

16.

Ice cream melting is an example of an __________ process.

a)

endothermic

b)

exothermic

17.

What is the specific heat of liquid water?

a)

4.184 J/gC

b)

1.00 J/gC

c)

0.129 J/gC

d)

2.44 J/gC

18.

What device is used to measure the amount of heat involved in a chemical reaction or physical process?

a)

barometer

b)

calorimeter

c)

thermometer

19.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

20.

The specific heat of a substance varies with the mass of a sample. True or False?

a)

True

b)

False

21.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

22.

The diagram represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

a)

Heat energy flows from solid A to solid B. Solid A decreases in temperature

b)

Heat energy flows from solid A to solid B. Solid A increases in temperature

c)

Heat energy flows from solid B to solid A. Solid B decreases in temperature.

d)

Heat energy flows from solid B to solid A. Solid B increases in temperature.

23.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

24.

When methane, CH4, and oxygen, O2, are mixed in a stove and ignited, a lovely blue flame results. The balanced equation is:

CH4(g) + 2O2(g) →\rightarrow 2H2O(g) + CO2(g)

What can be said about the energy involved in this chemical reaction?

I. The average kinetic energy of the products is greater than that of the reactants.

II. The chemical energy stored in the reactants is greater than the chemical energy stored in the products.

III. Chemical energy in the reactants is changed into heat energy and light energy.

a)

I only

b)

II only

c)

III only

d)

I, II, and III

25.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

26.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

27.
Durning a phase change the temperature of a substance_________.
a)
always increases
b)
always decreases
c)
always stays the same
d)
varies
28.

Match the following

a)

Specific Heat

1.

Energy required to change 1 gram of a substance by 1 degree celcius

b)

Heat

2.

Energy moving from higher temperature to lower

c)

Endothermic

3.

Chemical reaction where energy is absorbed

d)

Exothermic

4.

Chemical reaction where energy is released

e)

Chemical Energy

5.

Energy that is stored in chemical bonds/composition

29.

Reorder the following: The metals that take the least amount of energy to change the temperature to the highest amount

a)

Lead: 0.129

b)

Silver: 0.235

c)

Zinc: 0.385

d)

Iron: 0.444

e)

Aluminum: 0.900

1)
2)
3)
4)
5)
30.

Select all that apply for exothermic reactions

a)

Surroundings become cold

b)

Surroundings become hot

c)

Energy is absorbed

d)

Energy is released

e)

ΔH is negative

31.

A chemical reaction in a beaker causes the beaker to feel cold to the touch. What type of reaction occurred?

a)

endothermic

b)

exothermic

32.

Which of these is the unit for specific heat?

a)

J

b)

J/g

c)

J/goC

d)

oC

33.

Substance A heats more quickly than substance B. Which one has a higher specific heat?

a)

substance A

b)

substance B

c)

They have the same specific heat.

34.

A piece of aluminum with a mass of 20.0 grams is heated from 30 oC to 95 oC. If the specific heat of aluminum is 0.904 J/goC, how much heat is gained by the aluminum?

a)

1717.60 J

b)

1175.20 J

c)

963.68 J

d)

542.4 J

35.

A 300 gram sample of a metal is cooled from 120 oC to 60 oC, and releases 4230 J of energy. What is the specific heat of the metal?

a)

7.61 x 107 J/goC

b)

4.26 J/goC

c)

0.47 J/goC

d)

0.235 J/goC

36.

A 95 gram volume of water has an initial temperature of 30 oC. A piece of metal with a mass of 120 grams and an initial temperature of 98 oC is placed in the water. The final temperature of the water and the metal is 35 oC. What is the specific heat of the metal?

a)

7560 J/goC

b)

3.80 J/goC

c)

0.263 J/goC

d)

1987.4 J/goC

37.

4Fe(s) + 3O2(g) → 2Fe2O3(s) + 1625 kJ

Is this reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

38.

Is the reaction represented in this graph endothermic or exothermic?

a)

endothermic

b)

exothermic

39.
What kind of reaction is this?
a)

endothermic

b)
exothermic
40.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
41.
Which of the letters (A-D) represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
42.

Given the thermochemical equation, calculate the heat evolved when 74.6 g of sulfur dioxide (molar mass = 64.07 g/mol) is converted to sulfur dioxide.

a)

-115 kJ

b)

115 kJ

c)

-115.39 kJ

d)

115.39 kJ

43.

Calculate ΔH when 2 moles of ethanol (C2H5OH) reacts with excess oxygen according to the following thermochemical equation?

C2H5OH + 3O2 → 2CO2 + 3H2O ΔH = −1366.7 kJ

a)

-2733.4 kJ

b)

-683.35 kJ

c)

-1366.7 kJ

d)

-910.67 kJ

44.

What will ΔH be if there is 1 mole of oxygen?

4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1500 kJ

a)

-500 kJ

b)

500 kJ

c)

-750 kJ

d)

-4500 kJ

45.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
46.
Refer to the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
47.
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
48.

C+ O2 --> CO2 + 60kJ, what heat is released for the reaction if 3 moles of CO2 is formed?

a)

60 kJ

b)

120 kJ

c)

180 kJ

d)

20 kJ

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