1. Heating/Cooling Curve & Energy Calculations

2. Which of the following measures the average kinetic energy of a sample?
Mass
Volume
Specific heat
Temperature
Heat of fusion
Table

3. The flat lines on a heating curve represent…
A temperature change.
A constant state of matter.
A change in state.
A Change in average kinetic energy
Table

4. The sloped lines on a heating curve represent…
A constant temperature.
A change in state of matter.
A constant state of matter.
A constant value for the average kinetic energy
Table

5. Which portion of the curve represents the solid melting?1 2 3 4 5
Energy being added (cal)
500
200 60 10
Table

6. When does kinetic energy increase on a heating curve?
On the flat portions.
On the sloped lines.
Every point on the curve.
Table

7. What is enthalpy of fusion?
Amount of energy to raise temperature of 1g by 10
Amount of energy needed to boil 1g
Amount of energy needed to melt 1g
Table

8. What would be the freezing point temperature of this substance?
Not listed
Energy being added (cal)
500
200 60 10
Table

9. Which portion of the curve represents heating of the liquid?1 2 3 4 5
Energy being added (cal)
500
200 60 10
Response

10. For the same amount of heat added, a substance with a large specific heat…
Has a smaller increase in temp.
Has a larger increase in temp.
Has the same increase in temp.
Table

11. If the specific heat of ice is 0
If the specific heat of ice is 0.5 cal/gC°, how much heat would have to be added to 200 g of ice (solid water), initially at a temperature of -10°C, to raise the ice to the melting point?
1000 cal
-1000 cal
2000 cal
-2000 cal
Table

12. What is the specific heat of a metal if 24. 8 g absorbs 65
What is the specific heat of a metal if 24.8 g absorbs 65.7 cal of energy and the temperature rises from20.2 C to 24.5 C?
.62 cal/g C
78 cal/g C
66 cal/g C
Table

13. -23000 cal -21000 cal -20000 cal 2300 cal 2100 cal 20000 cal
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.
cal
cal
cal
2300 cal
2100 cal
20000 cal
Table