WorksheetsIPC Heat Equations
Total questions: 10
Worksheet time: 12mins
5.0 g of copper was heated from 20 C to 80 C. How much energy was used to heat Cu? The specific heat of copper is .385 J/gC
26.7 J
115.5 J
89.4 J
154.0 J
The energy from the sun causes the temperature of a granite boulder to change from 10 C to 29 C. If the boulder is 20g, how much heat did it absorb? The specific heat of granite is 0.79 J/gC.
399.2 J
200.2 J
453.6 J
300.2 J
If I have a 0.5g sample of copper and a 25g sample of copper, what is true about their specific heat values?
The specific heat increases as mass increases.
Specific heat is directly related to mass.
The specific heat does not change and is unique to each substance.
We need more information. Need to know temperature values.
Water has a high specific heat value. What does this mean about the substance?
It takes a small amount energy to raise the temperature.
It takes a lot of energy to change the temperature of 1g by 1 degree.
It changes its state of matter quickly
If the Q value (heat) is negative, what do we know about the substance?
Heat is released
Heat is absorbed
How much heat is released when 30 g of water at 96 degrees C cools to 25 degrees C? The specific heat of water is 4.18 J/gC
8903 J
3345 J
-12038 J
-8903 J
The specific heat of lead is 0.129 J/gC. A 8g sample of lead raises temperature by 15 degrees C. How much energy did it absorb?
15.5 J
32.8 J
-15.5 J
-14.6 J
What are the units for specific heat?
J/cal
J/g
cal/Jkg
J/gC
Looking at the table, which sample would require the most amount of energy to change the temperature?
Lead
Water
Ice
Copper
Based on the table, what do you know about lead?
Lead requires a lot of energy to raise the temperature.
Lead remains at a stable temperature for an extended amount of time.
Lead is more stable than water.
The temperature of lead can easily be raised.
