Chemistry
CH 10 Heat Calculations
Name ______
Period ______
Date______
- Heat problems where you are not changing states of matter.
- Calculate the nrgrequired to heat 200.0g of water from 5.0C to 35.0C.(25,080J)
- If 2500J is released during an exothermic process, calculate the mass of water needed to lower the temperature from 95.0C to 30.0C.(9.20g)
- If an endothermic process takes 1,500 J to heat up water. Calculate the final temperature of 150.0g of water starting at a temperature of 10.0C. (12.4C)
- Calculate the specific heat of 100.0g of an unknown liquid if 2,500J is released during the process of cooling down the unknown from 85.0C to 15.0C. (0.357J/gC)
- Heat problems where you are changing states of matter or changing phases.
- Calculate the nrg required to heat 150.0g of water at 25.0C to steam at 120.0C (392,115J)
- Calculate the Joules released when 25.0g of water cool from 105.0C to -15.0C (-76307.5 J)
- Given the following information about substance X, calculate the Joules required to raise 25.0g of substance X from 25.0C to 250.0C. (98,031.25 J)
MeltingPt = 15.0C BoilingPt = 200.0C Specific Heat Values Cpsolid =1.00J/gC Cpliquid = 2.05 J/gC Cpgas= 1.25J/gC Heat of Fusion = 250 J/g Heat of Vaporization = 3500 J/g
- Honors Chemistry Heat problems where you are mixing two substances but no phase changes
- Calculate the final temperature when you mix 100.0g of iron at 200.0C with 200.0g of water at 50.0C Cpiron as solid = 0.45 J/gC (57.7 C)
- Calculate thevolumeof water at 10.0C needed to mix with 100.0mL of water at 25.0C to cool the entire system down to 12.5C. (500.0 mL)
- Honors Chemistry Heat problems where you are mixing two substances and there are phase changes.
- Calculate the final temperature after mixing 25.0g of ice at -15.0C with 100.0 mL of water at 80.0C (46.6 C)
- Calculate the amount of ice needed at 0.0C to put into 200.0 mL of water to lower the temperature of the water 30.0C. The final temperature of the system at equilibrium is 0.0C (75.1 g)