1. Specific Heat
Q = m c ΔT

2. Q
Heat absorbed by a material
Measured in Joules (J)

3. m
Mass of the material
Measured in grams (g)

4. c
Specific heat, dependent upon the material
Measure in J/g°C

5. ΔT
Change in Temperature ΔT = Tfinal – Tinitial
Measured in °C

6. The temperature of 150 grams of water is raised from 20°C to 25°C
The temperature of 150 grams of water is raised from 20°C to 25°C. The specific heat of water is J/g°C. How much heat did the water gain?
Q Ra
I C F

7. How much heat is needed to raise the temperature of 100
How much heat is needed to raise the temperature of g of water by 85°C if the specific heat of water is J/g°C?
How much heat is absorbed by a 750-g iron skillet when its temperature is raised from 25°C to 125°C? The specific heat of iron is J/g°C.

8. You just set up a new aquarium with 75,000 g of water and need to raise the temperature by 3.8°C, how much heat is needed? The specific heat of water is 4.18 J/g°C.
Q Ra
I C F Q
m = 75,000 g
c = J/g°C
ΔT = 3.8 °C
Q = mc ΔT no
Q = mcΔT
= (75,000g)(4.18 J/g°C)(3.8°C)
= 1,191,300 J

9. 2. A jeweler is trying to release a diamond from its setting in a 10
2. A jeweler is trying to release a diamond from its setting in a 10.0 g silver ring. If the temperature has to change by 10.0°C, how much heat is needed? The specific heat of silver is J/g°C. Q Ra I C F Q
m = 10.0 g
c = J/g°C
ΔT = 10.0 °C
Q = mc ΔT no
Q = mcΔT
= (10.0 g)(0.235 J/g°C)(10.0°C)
= 23.5 J

10. 3. How much heat is needed to raise the temperature of 42 g of water by 3.0°C if the specific heat of water is 4.18 J/g°C? Q Ra I C F Q
m = 42 g
c = J/g°C
ΔT = 3.0 °C
Q = mc ΔT no
Q = mcΔT
= (42 g)(4.18 J/g°C)(3.0°C)
= J

11. 4. Gold has a specific heat of 0. 13 J/g°C
4. Gold has a specific heat of 0.13 J/g°C. If a sample of gold with a mass of 250 g undergoes a temperature increase of 4.0°C, how much heat does it absorb? Q Ra I C F Q
m = 250 g
c = J/g°C
ΔT = 4.0 °C
Q = mc ΔT no
Q = mcΔT
= (250g)(0.13 J/g°C)(4.0°C)
= 130 J

12. 5. A piece of iron at a temperature of 145°C cools off to a temperature of 45.0°C. If the iron has a mass of 10.0 g and a specific heat of J/g·°C, how much heat is given up? Q Ra I C F Q
m = 10.0 g
c = J/g°C
ΔT = 45°C - 145°C = -100°C
Q = mc ΔT no
Q = mcΔT
= (10.0g)(0.449 J/g°C)(-100°C)
= -449 J

13. 6. The specific heat of copper is 0. 39 J/g·°C
6. The specific heat of copper is 0.39 J/g·°C. How much heat is needed to raise the temperature of g of copper from 25°C to 45.0°C? Q Ra I C F Q
m = 1000 g
c = J/g°C
ΔT = 45°C - 20°C = 20°C
Q = mc ΔT no
Q = mcΔT
= (1000 g)(0.39 J/g°C)(20°C)
= 7800 J

14. 7. How much heat is absorbed by a 750 g iron skillet when its temperature rises from 25°C to 125°C? The specific heat of iron is J/g°C. Q Ra I C F Q
m = 750 g
c = J/g°C
ΔT = 125°C - 25°C = 100°C
Q = mc ΔT no
Q = mcΔT
= (750g)(0.449 J/g°C)(100°C)
= 33,675 J

15. 8. How much heat is needed to raise the temperature of 100
8. How much heat is needed to raise the temperature of g of water by 85.0°C? The specific heat of water is 4.18 J/g°C. Q Ra I C F no
Q = mcΔT
= (100g)(4.18 J/g°C)(85°C)
= 35,530 J Q
m = 100 g
c = J/g°C
ΔT = 85°C
Q = mc ΔT

16. 9. How much heat is given up when 450 g of water cool from 45°C to 20°C? The specific heat of water is 4.18 J/g°C. Q Ra I C F Q
m = 450 g
c = J/g°C
ΔT = 20°C - 45°C = -25°C
Q = mc ΔT no
Q = mcΔT
= (450g)(4.18 J/g°C)(-25°C)
= -47,025 J

17. Q = mcΔT What does each variable stand for?
Activator
Q = mcΔT What does each variable stand for?

18. You just set up a new aquarium with 45,000 g of water and need to raise the temperature by 2.5°C, how much heat is needed? The specific heat of water is 4.18 J/g°C.
Q Ra
I C F Q
m = 45,000 g
c = J/g°C
ΔT = 2.5 °C
Q = mc ΔT no
Q = mcΔT
= (45,000g)(4.18 J/g°C)(2.5°C)
= 470,250 J

19. 2. A jeweler is trying to release a diamond from its setting in a 8
2. A jeweler is trying to release a diamond from its setting in a 8.0 g silver ring. If the temperature has to change by 12.5°C, how much heat is needed? The specific heat of silver is J/g°C. Q Ra I C F Q
m = 8.0 g
c = J/g°C
ΔT = 12.5 °C
Q = mc ΔT no
Q = mcΔT
= (8.0 g)(0.235 J/g°C)(12.5°C)
= 23.5 J

20. 3. How much heat is needed to raise the temperature of 38 g of water by 5.5°C if the specific heat of water is 4.18 J/g°C? Q Ra I C F Q
m = 38g
c = J/g°C
ΔT = 5.5 °C
Q = mc ΔT no
Q = mcΔT
= (38g)(4.18 J/g°C)(5.5°C)
= J

21. 4. Gold has a specific heat of 0. 13 J/g°C
4. Gold has a specific heat of 0.13 J/g°C. If a sample of gold with a mass of 350 g undergoes a temperature increase of 14.0°C, how much heat does it absorb? Q Ra I C F Q
m = 350 g
c = J/g°C
ΔT = 14.0 °C
Q = mc ΔT no
Q = mcΔT
= (350g)(0.13 J/g°C)(14.0°C)
= 637 J

22. 5. A piece of iron at a temperature of 145°C cools off to a temperature of 45.0°C. If the iron has a mass of 10.0 g and a specific heat of J/g·°C, how much heat is given up? Q Ra I C F Q
m = 10.0 g
c = J/g°C
ΔT = 45°C - 145°C = -100°C
Q = mc ΔT no
Q = mcΔT
= (10.0g)(0.449 J/g°C)(-100°C)
= -449 J

23. 6. The specific heat of copper is 0. 39 J/g·°C
6. The specific heat of copper is 0.39 J/g·°C. How much heat is needed to raise the temperature of g of copper from 25°C to 45.0°C? Q Ra I C F Q
m = 1000 g
c = J/g°C
ΔT = 45°C - 20°C = 20°C
Q = mc ΔT no
Q = mcΔT
= (1000 g)(0.39 J/g°C)(20°C)
= 7800 J

24. 7. How much heat is absorbed by a 750 g iron skillet when its temperature rises from 25°C to 125°C? The specific heat of iron is J/g°C. Q Ra I C F Q
m = 750 g
c = J/g°C
ΔT = 125°C - 25°C = 100°C
Q = mc ΔT no
Q = mcΔT
= (750g)(0.449 J/g°C)(100°C)
= 33,675 J

25. 8. How much heat is needed to raise the temperature of 100
8. How much heat is needed to raise the temperature of g of water by 85.0°C? The specific heat of water is 4.18 J/g°C. Q Ra I C F no
Q = mcΔT
= (100g)(4.18 J/g°C)(85°C)
= 35,530 J Q
m = 100 g
c = J/g°C
ΔT = 85°C
Q = mc ΔT

26. 9. How much heat is given up when 450 g of water cool from 45°C to 20°C? The specific heat of water is 4.18 J/g°C. Q Ra I C F Q
m = 450 g
c = J/g°C
ΔT = 20°C - 45°C = -25°C
Q = mc ΔT no
Q = mcΔT
= (450g)(4.18 J/g°C)(-25°C)
= -47,025 J