Heating up
What is the formula for q that uses a substances specific heat capacity? (c)
q = mcΔT
What is the rearranged formula to solve for mass?
m = q/cΔT
What is the rearranged formula to solve for the specific heat capacity? (c)
c = q/mΔT
What is the rearranged formula to solve for the change in temperature? (ΔT)
ΔT = q/mc
What are the formulas for the heat of fusion and vaporization?
q = ΔHF ; q = ΔHV
What is the relationship between energy gained and energy lost?
qgained = -qlost
Joules (J) or calories (cal)
If an object's mass is doubled, what will happen to the amount of energy necessary to raise the temperature by the same amount?
Specific heat capacity is measured in what units?
J/goC
What is the formula to calculate for ΔT if you are given the initial and final temperature?
ΔT = TF - TI
What is the heat of fusion of a 25.0 g sample of water at 0.00 C? (Hf = 334 J/g)
8,350 J
If hot metal is placed in cool water and loses 10,000 J, how much energy did the water gain?
10,000 J
What energy in J would it take to heat 5.00 g of water from 25.0C to 35.0C? (c = 4.18 J/gC)
209 J
What mass of oxygen would be heated 5000.0 J if the ΔT was 300.C? (c = 0.918 J/gC)
m = 18.2 g
What is the specific heat of a substance with 50.0 g of mass, 5000. J added, and a ΔT of 45.0C?
2.22 J/gC
What is the ΔT of glass with 20.0 g of mass and 800. J added? (c = 0.840 J/gC)
47.6 C
What is the heat of fusion of a 52.0 g sample of water at 100. C? (Hv = 2260 J/g)
118,000 J
What would be the heat energy if 15.0 g of iron were cooled from 400.C to 50.0C? (c = 0.412 J/gC)
q = -2160 J
What mass of water would be heated 4500.0 J if the starting temperature was 15.0 C and final temp was 100.C? (c = 0.918 J/gC)
57.7 g
What is the specific heat of a substance with 53.0 g of mass, 3400. J added, and an initial temp of 12.0C, final temp 48.0C?
1.78 J/gC
What is the ΔT of brass with 98.3 g of mass and 9840. J added? (c = 0.380 J/gC)
263 C
What is the total energy needed to melt 35.0 g water starting at -15 C? (Hf = 334 J/g) (c = 2.08 J/gC)
11,700 J + 1090 J = 12,790 J
Which would require more heat energy? Heating 20.0 g of water from 25.0C to 75.0C, or 40.0 g of water from 25.0C to 60.0C? (c = 4.18 J/gC)
20g q = 4180 J
40g q = 5850 J
What mass of silver would be cooled with the release of 2000.0 J if the initial temp was 250.C and the final was 20.0C? (c = 0.233 J/gC)
37.3 g
What is the specific heat of a substance with 77.2 g of mass, 12000. J added, and an initial temp of 10.0C, final temp 480.0C?
0.331 J/gC
What is the FINAL temperature of an aluminum sample with 402.0 g of mass and 76490. J added if the initial temp is 25.2 C? (c = 0.897 J/gC)
237 C
What is the total energy needed to vaporize 53.0 g water starting at 30.0 C? (Hf = 2260 J/g) (c = 4.18 J/gC)
15,500 J + 120,000 J = 135,500 J
What is the mass of water that would cool 54.0 g of iron (c = 0.412) from 400. to 30.0 C? The starting temp of the water was 25.0 C. (c of water = 4.18)
394 g