Heating/Cooling Curve&

Energy Calculations

Which of the following measures the average kinetic energy of a sample?

1. 2. 3. 4. 5.

0% 0% 0%0%0%

1. Mass2. Volume3. Specific heat4. Temperature5. Heat of fusion

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The flat lines on a heating curve represent…

1. 2. 3. 4.

0% 0%0%0%

1. A temperature change.2. A constant state of matter.3. A change in state.4. A Change in average kinetic energy

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The sloped lines on a heating curve represent…

1. 2. 3. 4.

0% 0%0%0%

1. A constant temperature.2. A change in state of matter.3. A constant state of matter.4. A constant value for the average kinetic

energy

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Which portion of the curve represents the solid melting?

0%

0%

0%

0%

0% 1. 12. 23. 34. 45. 5

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Energy being added (cal)

500

200

60

10

0

When does kinetic energy increase on a heating curve?

1. 2. 3.

0% 0%0%

1. On the flat portions.2. On the sloped lines.3. Every point on the curve.

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What is enthalpy of fusion?

1. 2. 3.

0% 0%0%

1. Amount of energy to raise temperature of 1g by 10

2. Amount of energy needed to boil 1g3. Amount of energy needed to melt 1g

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What would be the freezing point temperature of this substance?

0%

0%

0%

0%

0%

0% 1. 0 °C2. 10 °C3. 60 °C4. 200 °C5. 500 °C6. Not listed

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Energy being added (cal)

500

200

60

10

0

Which portion of the curve represents heating of the liquid?

0%

0%

0%

0%

0% 1. 12. 23. 34. 45. 5

Energy being added (cal)

500

200

60

10

0Response

For the same amount of heat added, a substance with a large specific heat…

1. 2. 3.

0% 0%0%

1. Has a smaller increase in temp.2. Has a larger increase in temp.3. Has the same increase in temp.

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If the specific heat of ice is 0.5 cal/gC°, how much heat would have to be added to 200 g of ice, initially at a temperature of -10°C, to raise the ice to the melting point?

1. 2. 3. 4.

0% 0%0%0%

1. 1000 cal2. -1000 cal3. 2000 cal4. -2000 cal

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What is the specific heat of a metal if 24.8 g absorbs65.7 cal of energy and the temperature rises from20.2 C to 24.5 C?

1. 2. 3.

0% 0%0%

1. .62 cal/g C 2. 78 cal/g C 3. 66 cal/g C

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A hot-water bottle contains 750 g of water at 65 °C. If the water cools to body temperature (37 °C), calculate the energy transfer experienced by the water in the hot water bottle.

1. 2. 3. 4. 5. 6.

0% 0% 0%0%0%0%

1. -23000 cal2. -21000 cal3. -20000 cal4. 2300 cal5. 2100 cal6. 20000 cal

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