Chapter 6 Question Preview (ID: 50530)
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What happens to the energy produced by burning gasoline in a car engine?
a) The energy is lost as heat in the exhaust
b) The energy is transformed into work to move the car
c) The energy heats the parts of the engine
d) All of the above
A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?
a) The temperature of the metal will increase
b) The temperature of the water will increase.
c) The temperature of the water will decrease.
d) The temperature of the water will increase and the temperature of the metal will decrease.
What would likely happen if you were to touch the flask in which an endothermic reaction were occurring?
a) The flask would probably feel cooler than before the reaction started
b) The flask would probably feel warmer than before the reaction started.
c) The flask would feel the same as before the reaction started
d) None of the above
The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as
a) a joule
b) specific heat
c) a calorie
d) density
When energy is changed from one form to another, ____
a) some of the energy is lost entirely
b) all of the energy can be accounted for
c) a physical change occurs
d) all of the energy is changed to a useful form
If heat is released by a chemical system, an equal amount of heat will be ____.
a) absorbed by the surroundings
b) absorbed by the universe
c) released by the surroundings
d) released by the universe
Which of the following is transferred due to a temperature difference?
a) chemical energy
b) mechanical energy
c) electrical energy
d) heat
In an exothermic reaction, the energy stored in the chemical bonds of the reactants is ____.
a) equal to the energy stored in the bonds of the products
b) greater than 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
A process that absorbs heat is a(n) ____.
a) endothermic process
b) polythermic process
c) exothermic process
d) ectothermic process
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 more heat
b) The body releases less heat
c) The body releases the same amount of heat.
d) The body releases no heat.
The heat capacity of an object depends in part on its ____.
a) mass
b) enthalpy
c) shape
d) potential energy
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) less than the specific heat of water
c) equal to the specific heat of water
d) Not enough information is given.
Which of the following has the greatest heat capacity?
a) 1000 g of water
b) 1000 g of steel
c) 1 g of water
d) 1 g of steel
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 volume
c) its temperature
d) its energy
The amount of heat transferred from an object depends on which of the following?
a) the specific heat of the object
b) the initial temperature of the object
c) the mass of the object
d) all of the above
What does the symbol ∆H stand for?
a) the specific heat of a substance
b) the heat capacity of a substance
c) the heat of reaction for a chemical reaction
d) one Calorie given off by a reaction
The amount of heat released by the complete burning of 1 mole of a substance is the ____.
a) specific heat
b) heat of combustion
c) heat of capacity
d) heat of fusion
The heat content of a system is equal to the enthalpy only for a system that is at constant ____.
a) Temperature
b) volume
c) pressure
d) mass
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 released per mole
b) 88.0 kJ released per mole
c) 88.0 kJ absorbed per mole
d) 216.8 kJ absorbed per mole
What is the heat of solution?
a) the amount of heat required to change a solid into a liquid
b) the amount of heat absorbed or released when a solid dissolves
c) the amount of heat required to change a vapor into a liquid
d) the amount of heat released when a vapor changes into a liquid
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