Heating/Cooling Curve
&
Energy Calculations
Which of the following measures the
average kinetic energy of a sample?
1.
2.
3.
4.
5.
Mass
Volume
Specific heat
Temperature
Heat of fusion
Table
0%
1.
0%
0%
2.
3.
0%
0%
4.
5.
The flat lines on a heating curve
represent…
1.
2.
3.
4.
A temperature change.
A constant state of matter.
A change in state.
A Change in average kinetic energy
Table
0%
1.
0%
2.
0%
3.
0%
4.
The sloped lines on a heating curve
represent…
1.
2.
3.
4.
A constant temperature.
A change in state of matter.
A constant state of matter.
A constant value for the average kinetic
energy
Table
0%
1.
0%
2.
0%
3.
0%
4.
Which portion of the curve represents
the solid melting?
0%
0%
0%
0%
0%
1.
2.
3.
4.
5.
1
2
3
4
5
500
200
60
Table
10
0
Energy being added (cal)
When does kinetic energy increase on
a heating curve?
1. On the flat portions.
2. On the sloped lines.
3. Every point on the curve.
Table
0%
1.
0%
2.
0%
3.
What is enthalpy of fusion?
1. Amount of energy to raise temperature of 1g
by 10
2. Amount of energy needed to boil 1g
3. Amount of energy needed to melt 1g
Table
0%
1.
0%
2.
0%
3.
What would be the freezing point
temperature of this substance?
0%
0%
0%
0%
0%
0%
1.
2.
3.
4.
5.
6.
0 °C
10 °C
60 °C
200 °C
500 °C
Not listed
500
200
60
10
0
Table
Energy being added (cal)
Which portion of the curve represents
heating of the liquid?
0%
0%
0%
0%
0%
1.
2.
3.
4.
5.
1
2
3
4
5
500
200
60
10
Response
0
Energy being added (cal)
For the same amount of heat 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
0%
1.
0%
2.
0%
3.
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, initially at a temperature of -10°C, to
raise the ice to the melting point?
1.
2.
3.
4.
1000 cal
-1000 cal
2000 cal
-2000 cal
Table
0%
1.
0%
2.
0%
3.
0%
4.
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
0%
1.
0%
2.
0%
3.
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.
-23000 cal
-21000 cal
-20000 cal
2300 cal
2100 cal
20000 cal
Table
0%
0%
0%
0%
0%
0%
1.
2.
3.
4.
5.
6.