1. Heating Curves and Energy

2. Which of the following measures the average kinetic energy of a sample? 1.Mass 2.Volume 3.Specific heat 4.Temperature 5.Heat of fusion Table

3. The flat lines ( )on a heating curve represent… 1.A temperature change. 2.A constant state of matter. 3.A change in state. 4.A Change in average kinetic energy Table

4. The sloped lines( or ) on a heating curve represent… 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 Table

5. Which portion of the curve represents the solid melting? 1.1 2.2 3.3 4.4 5.5 Table

6. When does kinetic energy change on a heating curve? 1.On the flat portions. 2.On the sloped lines. 3.Every point on the curve. Table

7. If the specific heat of ice (solid water) is 0.5 cal/g  C°, 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 (0°C)? 1.1000 cal 2.-1000 cal 3.2000 cal 4.-2000 cal Table

8. What is enthalpy (heat) of fusion? 1.Amount of energy to raise temperature of 1g of a substance by 1 0 2.Amount of energy needed to boil (turn to gas) 1g of a substance 3.Amount of energy needed to melt (turn to liquid) 1g of a substance Table

9. Which portion of the curve represents heating of the liquid? 1.1 2.2 3.3 4.4 5.5 Table

10. For the same amount of heat (energy) added, a substance with a large specific heat… 1.Has a smaller increase in temp. 2.Has a larger increase in temp. 3.Has the same increase in temp. Table

11. What is the specific heat of a metal if 24.8 g absorbs 65.7 cal of energy and the temperature rises from 20.2  C to 24.5  C? 1..62 cal/g  C 2.78 cal/g  C 3.66 cal/g  C Table

12. A hot-water bottle contains 750 g of water at 65 °C. If the water cools to body temperature (37 °C), Calculate the energy change for the water. 1.-23000 cal 2.-21000 cal 3.-20000 cal 4.23000 cal 5.21000 cal 6.20000 cal Table