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WorksheetsSpecific Heat Capacity and Phase Changes
Total questions: 15
Worksheet time: 28mins
What is specific heat capacity?
The amount of heat required to raise the temperature of one gram of a substance by 1°C
The amount of radiant energy required to increase the temperature of one gram of a substance by 1°C
The amount of energy required to increase the temperature of one gram of a substance by 1°C
The amount of friction required to increase the temperature of one gram of a substance by 1°C
The specific heat of platinum is 0.133 J/g°C. How much heat is released when a 10.0 g piece of platinum cools from 100.0°C to 50.0°C?
-66.5 J
-665 J
-0.0266 J
-0.665 J
Calculate the amount of energy required to melt 35 grams of ice. ΔHf = 80.0 cal/g, ΔHv = 560.0 cal/g, c = 1.00 cal/gºC
19,000 cal
35 cal
2,800 cal
1,600,000 cal
How much heat moves from the water to the surroundings when 20.0 g of water is heated from 20.0°C to 25.0°C? The specific heat of water is 4.184 J/g°C.
418 J
209 J
83.0 J
4.18 J
Energy, per amount, absorbed or released when a substance melts or freezes is called
Heat of vaporization
Heat of deposition
Heat of fusion
Heat of sublimation
The specific heat of copper is 0.39 J/g °C. What is the temperature change when 100. Joules of heat is added to 20.0 grams?
1.85°C
24.1°C
12.8°C
5130°C
The specific heat of water is 4.184 J/g°C, and the specific heat of wood is 1.760 J/g°C. Which material needs more heat to raise the temperature?
Water
Wood
Both are same
A substance with a low specific heat heats up __________, while a substance with a high specific heat heats up __________.
Slowly, quickly
Quickly, slowly
The temperature of an unknown piece of metal with a mass of 30.0 g changes from 25.0°C to 35.0°C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?
1.17 J/g°C
-1.17 J/g°C
0.857 J/g°C
-0.857 J/g°C
What is the formula used to calculate the heat required to raise the temperature of any substance?
Q=mc
Q=mc∆t
Q= ½mv
m=QC
How many Joules of energy are required to make 0.100 kg of ice at 0.0°C completely melts? The heat of fusion of ice is 334,000 J/kg.
255 J
400. J
33,400 J
2,460,000 J
During a phase change, temperature
Increases
Decreases
Does not change
A pot of water at a temperature of 25.0°C is heated on a stove until the water boils (100.0°C), which requires 750,000 J of energy. What is the mass of the water in the pot? The specific heat of water is 4.184 J/g°C.
13 g
2,400 g
120 g
1,500 g
How much energy is required to completely boil 150. g of water? c = 4.184 J/gºC and ΔHv = 2260 J/g
56,500 J
339,000 J
395,000 J
85,400 J
Energy, per amount, absorbed or released when a substance vaporizes or condenses
Heat of vaporization
Heat of deposition
Heat of fusion
Heat of sublimation
