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Intro Thermochemistry Notes Practice

Total questions: 50

Worksheet time: 3hrs 40mins

Name
Class
Date
1.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
2.
Hot coffee is stirred with a spoon; the spoon gets hot due to
a)
conduction
b)
convection
c)
radiation
3.
"Lava lamps" contain colored liquids. These liquids form globs that rise to the top due to
a)
conduction
b)
convection
c)
radiation
4.

Which law states that energy cannot be created nor destroyed, but it can be transformed or transferred?

a)

Dalton's Law

b)

law of conservation of energy

c)

Hess's Law

d)

E=mc^2

5.

What happens when kinetic energy increases?

a)

Temperature increases.

b)

Temperature decreases.

c)

Temperature is not affected by kinetic energy.

6.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

7.

In an exothermic reaction, heat is a...

a)

product (released)

b)

reactant (absorbed)

8.

If you touch an endothermic reaction, it will feel...

a)

hot

b)

cold

9.

The graph is showing an ____________ reaction.

a)

exothermic

b)

endothermic

10.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

11.
Describe the substance between letters E and F. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
12.

Entropy is a measure of

a)

accuracy

b)

precision

c)

the disorder of a system

d)

the attraction of a nucleus for an electron

13.

Quantity of heat needed to change the temperature of 1 g of a substance by 1 °C

a)

Heat capacity

b)

Calorie

c)

Joule

d)

Enthalpy

e)

Specific heat

14.

Which letter on the diagram represents a solid?

a)

A

b)

B

c)

C

d)

D

15.

Which letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

16.
Which way does heat flow?
a)
hot to cold
b)
cold to hot
c)
it doesn't 
17.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
18.
Heat travels from the sun to the earth by the process of...
a)
conduction
b)
convection
c)
radiation
d)
insulation
19.
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
20.

Which law of thermodynamics establishes absolute zero as the temperature at which the entropy of a system is zero?

a)

1st law of thermodynamics

b)

2nd law of thermodynamics

c)

3rd law of thermodynamics

d)

Zeroth Law

21.

What is the metric unit for heat?

a)

joules

b)

grams

c)

degrees celsius

d)

calories

22.

The first law of thermodynamics states that energy is

a)

created

b)

destroyed

c)

conserved

d)

created and destroyed

23.

What does ΔH symbolize?

a)

Enthalpy

b)

Entropy

c)

Energy

d)

Matter

24.

What device measures the change of energy for a system?

a)

thermometer

b)

calorimeter

c)

spectrometer

d)

pH meter

25.

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.

26.

Vaporization is what kind of change?

a)
Endothermic
b)
Exothermic
27.
Condensation and raining are examples of what?
a)
Exothermic
b)
Endothermic
28.

__________ is the transfer of heat by the movement of a fluid.

a)

Conduction

b)

Convection

c)

Radiation

29.

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

30.

What unit do you use to measure Thermal Energy?

a)

J/g ºC

b)

g

c)

ºC

d)

J

31.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
32.
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
33.

Water has a specific heat of 4.184 J/gºC. Wood has a specific heat of 1.760 J/gºC. What material needs more energy to raise the temperature by 1ºC

a)

Wood

b)

Water

c)

Both are the same

34.

How many Joules of energy are required to change 10 gram of liquid water from 20 C to 90 C? (specific heat of water=4.184 J/gC)

a)

1400 J

b)

2900 J

c)

210,000 J

d)

1,400,000 J

35.

If the specific heat of water is 4.184 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

112,575.9 K

36.

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

37.

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, requiring more energy to heat up than water.

b)

Sand has a lower specific heat than water, requiring less energy to heat up than water.

c)

Sand has a greater mass than water.

d)

Water has a greater mass than sand.

38.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
39.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
40.

In the Image, will the heat (+177.8 KJ) be a product or a reactant?

a)

Product

b)

Reactant

41.

In the Image, will the heat (-890.4 KJ KJ) be a product or a reactant?

a)

Product

b)

Reactant

42.

What is the sign of ΔH for an exothermic reaction?

a)

Positive

b)

Negative

c)

Zero

d)

Undefined

43.

Which process has a negative ΔH?

a)

Evaporation

b)

Melting

c)

Sublimation

d)

Condensation

44.

Breaking bonds is _________________. Forming bonds is ______________________

a)

endothermic, exothermic

b)

exothermic, endothermic

45.

The mass of a sample is 30g. There’s a temperature change from 18°C to 35°C when it absorbed 625 J of heat. What is the specific heat of this sample?

a)

2.78 J/g•°C

b)

8.67 J/g•°C

c)

1.23 J/g•°C

d)

108.67 J/g•°C

46.
Conversion Factor  1 cal = ____J
a)
10
1000
b)
1
c)
4.184
d)
4184
47.
Convert 350 J = ______ calories
a)
1464.4
b)
83.65
c)
0.350
d)
none of the above
48.
Convert 250 cal = ______ Joules
a)
1,046
b)
59.75
c)
0.250
d)
none of the above
49.
Conversion Factor 1kcal = ___ cal
a)
10
b)
100
c)
1000
d)
1/1000
50.

Convert 2.5 kcal = ____J (convert Kcal to cal first!)

a)
2500
b)
0.0025
c)
10,460
d)
10.46

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