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Chapter 6
Test Description: For activitiy online during MCO Covid19
Instructions: Answer all questions to get your test result.
1) What happens to the energy produced by burning gasoline in a car engine?
A
The energy heats the parts of the engine
B
All of the above
C
The energy is transformed into work to move the car
D
The energy is lost as heat in the exhaust
2) A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?
A
The temperature of the water will increase and the temperature of the metal will decrease.
B
The temperature of the water will increase.
C
The temperature of the water will decrease.
D
The temperature of the metal will increase
3) What would likely happen if you were to touch the flask in which an endothermic reaction were occurring?
A
None of the above
B
The flask would probably feel cooler than before the reaction started
C
The flask would probably feel warmer than before the reaction started.
D
The flask would feel the same as before the reaction started
4) The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as
A
a calorie
B
a joule
C
density
D
specific heat
5) When energy is changed from one form to another, ____
A
all of the energy is changed to a useful form
B
all of the energy can be accounted for
C
some of the energy is lost entirely
D
a physical change occurs
6) If heat is released by a chemical system, an equal amount of heat will be ____.
A
released by the surroundings
B
absorbed by the surroundings
C
released by the universe
D
absorbed by the universe
7) Which of the following is transferred due to a temperature difference?
A
heat
B
chemical energy
C
mechanical energy
D
electrical energy
8) In an exothermic reaction, the energy stored in the chemical bonds of the reactants is ____.
A
greater than the energy stored in the bonds of the products
B
equal to the energy stored in the bonds of the products
C
less than the energy stored in the bonds of the products
D
less than the heat released
9) A process that absorbs heat is a(n) ____.
A
endothermic process
B
ectothermic process
C
exothermic process
D
polythermic process
10) When your body breaks down sugar completely, how much heat is released compared to burning the same amount of sugar in a flame?
A
The body releases less heat
B
The body releases the same amount of heat.
C
The body releases no heat.
D
The body releases more heat
11) The heat capacity of an object depends in part on its ____.
A
mass
B
potential energy
C
enthalpy
D
shape
12) How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7 g of olive oil by 30°C?
A
greater than the specific heat of water
B
Not enough information is given.
C
equal to the specific heat of water
D
less than the specific heat of water
13) Which of the following has the greatest heat capacity?
A
1000 g of steel
B
1000 g of water
C
1 g of water
D
1 g of steel
14) By what quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
A
its mass
B
its energy
C
its volume
D
its temperature
15) The amount of heat transferred from an object depends on which of the following?
A
all of the above
B
the initial temperature of the object
C
the mass of the object
D
the specific heat of the object
16) What does the symbol ∆H stand for?
A
one Calorie given off by a reaction
B
the specific heat of a substance
C
the heat capacity of a substance
D
the heat of reaction for a chemical reaction
17) The amount of heat released by the complete burning of 1 mole of a substance is the ____.
A
heat of capacity
B
heat of fusion
C
heat of combustion
D
specific heat
18) The heat content of a system is equal to the enthalpy only for a system that is at constant ____.
A
pressure
B
Temperature
C
volume
D
mass
19) What is the standard heat of reaction for the following reaction? Zn(s) + Cu2+ (aq) → Zn2 + (aq) + Cu(s) ∆Hf ( Cu2+) = +64.4 kJ/mol; ∆H (Zn2 + ) = –152.4 kJ/mol)
A
216.8 kJ absorbed per mole
B
88.0 kJ released per mole
C
216.8 kJ released per mole
D
88.0 kJ absorbed per mole
20) What is the heat of solution?
A
the amount of heat required to change a vapor into a liquid
B
the amount of heat released when a vapor changes into a liquid
C
the amount of heat required to change a solid into a liquid
D
the amount of heat absorbed or released when a solid dissolves
*select an answer for all questions
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