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WorksheetsThermochemistry Test Review
Total questions: 45
Worksheet time: 1hrs 16mins
Name
Class
Date
1.
A kind of energy stored in an object for later use is
a)
kinetic energy
b)
potential energy
c)
mechanical energy
d)
nuclear energy
2.
6.42 Joules (J) to calories (cal)
a)
6420 cal
b)
.00642 cal
c)
1.5 cal
d)
24 cal
3.
Convert 120 Cal to Joules
a)
.502 Joules
b)
502080 Joules
c)
502 Joules
4.
What has particularly high specific heat?
a)
Water
b)
Gases
c)
Metals
d)
Poptarts
5.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
6.
For the formula:
Q= m c ∆T
The units for specific heat are:
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
7.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
8.
Thermal energy ALWAYS moves from _____ to _____.
a)
solid to liquid
b)
ice to water
c)
hot to cold
d)
solid to gas
9.
To measure the temperature difference between two cups of water, you would use a _____.
a)
measuring cup
b)
ruler
c)
thermometer
d)
balance scale
10.
What has particularly high specific heat?
a)
Water
b)
Gases
c)
Metals
d)
Poptarts
11.
How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
12.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
13.
When iron nails get rusty, heat is released. What process is this?
a)
Exothermic
b)
Endothermic
14.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
15.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
16.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______.
a)
Warm
b)
Cold
17.
What information do we get from calorimetry?
a)
How much food costs
b)
How much energy is in a food sample
c)
How many nutrients are in a food sample
d)
How much water is in food
18.
Where is the energy stored in a compound?
a)
Atoms
b)
Bonds
19.
Energy that is stored in bonds between atoms is:
a)
Mechanical energy
b)
Chemical energy
c)
Kinetic energy
d)
Nuclear energy
20.
Heat is measured in
a)
joules
b)
grams
c)
degrees celcius
21.
The Law of _______________ states that energy cannot be created nor destroyed only transferred
a)
Specific Heat
b)
Conservation of Energy
c)
Exothermic Reaction
d)
Potential Energy
22.
Refer to the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
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
23.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
24.
A material was cooled from 100ºC to 40ºC. What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
25.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
26.
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
27.
The specific heat of aluminum is 0.21 cal/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
28.
There are four cups of hot cocoa. The cup sizes are shown. The temperature of the cocoa in each cup is 25 degrees celsius. Which cup has the MOST thermal energy?
a)
Large cup (Trenta)
b)
Small cup (Tall)
c)
Venti
d)
All three are the same temperature so they have same thermal energy
29.
Amount of energy required to increase the temperatureof 1 g of water by 1"C
a)
calorie
b)
joule
c)
Calorie
d)
kcal
30.
a)
Aluminum
b)
Copper
c)
Gold
d)
Not enough information to answer the question.
31.
Exothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
32.
___________________ is the average kinetic energy of the particles of a substance.
a)
volume
b)
temperature
c)
mass
d)
length
33.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
34.
Represented with a "q"
a)
Work
b)
Heat
c)
Temperature
35.
500 joules = __________ calories
a)
2092
b)
119.50
c)
5418.4
d)
918.4
36.
What happens to the bonds when 2 substances react
a)
They break so new bonds can form
b)
Nothing the bonds are too strong
c)
They change colour
37.
The capacity to do work or transfer heat
a)
temperature
b)
energy
c)
power
d)
enthalpy
38.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
39.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
40.
A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils (100˚C). The specific heat of water is 4.184 J/(g˚C). Determine the heat energy needed to heat the water in the pot to boiling.
a)
133.76J
b)
43,062.2J
c)
753120
d)
1,003,200J
41.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
42.
A Big Mac has 563 food Calories. How many joules of energy are in a Big Mac?
a)
135 joules
b)
2360 joules
c)
135000000 joules
d)
2360000 joules
43.
For the following reaction, C(s){graphite}+O2(g)→CO2(g) ΔH=−393.41 kJ/mol
you have 45.6g of graphite. What is the heat of that reaction?
a)
-347.81 kJ
b)
-8.62 kJ
c)
-393.41 kJ
d)
-1490 kJ
44.
Condensation is
a)
Endothermic
b)
Exothermic
c)
Both Endothermic and Exothermic
d)
Can be either Endothermic or Exothermic
45.
Melting is
a)
Endothermic
b)
Exothermic
c)
Both Endothermic and Exothermic
d)
Can be either Endothermic or Exothermic
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