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Chapter 17 Test - Section 17.1 & 17.3



Multiple Choice (Value 28) 1 Bonus Question
Identify the choice that best completes the statement or answers the question.
 

 1. 

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
 

 2. 

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.
 

 3. 

How does a calorie compare to a joule?
a.
A calorie is smaller than a joule.
c.
A calorie is equal to a joule.
b.
A calorie is larger than a joule.
d.
The relationship cannot be determined.
 

 4. 

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
 

 5. 

Which of the following is NOT a form of energy?
a.
light
c.
heat
b.
pressure
d.
electricity
 

 6. 

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
 

 7. 

If heat is released by a chemical system, an equal amount of heat will be ____.
a.
absorbed by the surroundings
c.
released by the surroundings
b.
absorbed by the universe
d.
released by the universe
 

 8. 

Which of the following is transferred due to a temperature difference?
a.
chemical energy
c.
electrical energy
b.
mechanical energy
d.
heat
 

 9. 

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
 

 10. 

A process that absorbs heat is a(n) ____.
a.
endothermic process
c.
exothermic process
b.
polythermic process
d.
ectothermic process
 

 11. 

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.
 

 12. 

The quantity of heat required to change the temperature of 1 g of a substance by 1mc012-1.jpgC is defined as ____.
a.
a joule
c.
a calorie
b.
specific heat
d.
density
 

 13. 

A piece of candy has 5 Calories (or 5000 calories). If it could be burned, leaving nothing but carbon dioxide and water, how much heat would it give off?
a.
500 calories
c.
5000 joules
b.
5 kilocalories
d.
Not enough information is given.
 

 14. 

How many joules are in 148 calories? (1 cal = 4.18 J)
a.
6.61 J
c.
148 J
b.
35.4 J
d.
619 J
 

 15. 

What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10mc015-1.jpgC? (specific heat of aluminum = 0.21 mc015-2.jpg)
a.
420 cal
c.
42,000 cal
b.
4200 cal
d.
420,000 cal
 

 16. 

What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample by 15mc016-1.jpgC?
a.
0.033 mc016-2.jpg
c.
0.99 mc016-4.jpg
b.
0.33 mc016-3.jpg
d.
1.33 mc016-5.jpg
 

 17. 

How many kilocalories of heat are required to raise the temperature of 225 g of aluminum from 20mc017-1.jpgC to 100mc017-2.jpgC? (specific heat of aluminum = 0.21 mc017-3.jpg)
a.
0.59 kcal
c.
85 kcal
b.
3.8 kcal
d.
none of the above
 

 18. 

The heat capacity of an object depends in part on its ____.
a.
mass
c.
shape
b.
enthalpy
d.
potential energy
 

 19. 

Which of the following is a valid unit for specific heat?
a.
mc019-1.jpg
c.
mc019-2.jpg
b.
cal
d.
mc019-3.jpgC
 

 20. 

When 45 g of an alloy, at 25mc020-1.jpgC, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37mc020-2.jpgC, what is its specific heat?
a.
0.423 mc020-3.jpg
c.
9.88 mc020-5.jpg
b.
1.77 mc020-4.jpg
d.
48.8 mc020-6.jpg
 

 21. 

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 30mc021-1.jpgC?
a.
greater than the specific heat of water
c.
equal to the specific heat of water
b.
less than the specific heat of water
d.
Not enough information is given.
 

 22. 

The specific heat of silver is 0.24 mc022-1.jpg. How many joules of energy are needed to warm 4.37 g of silver from 25.0mc022-2.jpgC to 27.5mc022-3.jpgC?
a.
2.62 J
c.
45.5 J
b.
0.14 J
d.
0.022 J
 

 23. 

Which of the following has the greatest heat capacity?
a.
1000 g of water
c.
1 g of water
b.
1000 g of steel
d.
1 g of steel
 

 24. 

Which of the following substances has the highest specific heat?
a.
steel
c.
alcohol
b.
water
d.
chloroform
 

 25. 

By what quantity must the heat capacity of an object be divided to obtain the specific heat of that material?
a.
its mass
c.
its temperature
b.
its volume
d.
its energy
 

 26. 

The heat content of a system is equal to the enthalpy only for a system that is at constant ____.
a.
temperature
c.
pressure
b.
volume
d.
mass
 

 27. 

On what principle does calorimetry depend?
a.
Hess's law
c.
law of enthalpy
b.
law of conservation of energy
d.
law of multiple proportions
 

 28. 

How can the enthalpy change be determined for a reaction in an aqueous solution?
a.
by knowing the specific heat of the reactants
b.
by mixing the reactants in a calorimeter and measuring the temperature change
c.
by knowing the mass of the reactants
d.
The enthalpy change for this type of reaction cannot be determined.
 

 29. 

A chunk of ice whose temperature is –20mc029-1.jpgC is added to an insulated cup filled with water at 0mc029-2.jpgC. What happens in the cup?
a.
The ice melts until it reaches the temperature of the water.
b.
The water cools until it reaches the temperature of the ice.
c.
Some of the water freezes, so the chunk of ice gets larger.
d.
none of the above
 

Short Answer (Value 3)
 

 30. 

If 500 g of iron absorbs 22,000 cal of heat, what will be the change in temperature? (specific heat of iron = 0.11 sa030-1.jpg)  Formula q = mcÄt
 



 
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