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Heating Curves and Energy. Which of the following measures the average kinetic energy of a sample? 1.Mass 2.Volume 3.Specific heat 4.Temperature 5.Heat.

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Presentation on theme: "Heating Curves and Energy. Which of the following measures the average kinetic energy of a sample? 1.Mass 2.Volume 3.Specific heat 4.Temperature 5.Heat."— Presentation transcript:

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


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