Standard: Students know how to solve problems involving heat flow and temperature changes, using known values of specific heat and latent heat of phase change.
How many joules are required to heat 150 grams of water from 20 ºC to 35 ºC? The specific heat of water is 4.18 J/(g·ºC).
2000 joules are required to heat 125 grams of an unknown substance from 10 ºC to 28 ºC. What is the specific heat of the substance?
A 95 gram piece of a metal at 21 ºC absorbs 1000 J of energy, after which the temperature of the metal is 38 ºC. What is the specific heat of the metal?
How many joules are required to heat 38 grams of gold from 60 ºC to 260 ºC? The specific heat of gold is 0.129 J/(g·ºC).
When 1045 joules are absorbed by a certain mass of water, the temperature of the water increases from 45 ºC to 50 ºC. What is the mass of the water sample? The specific heat of water is 4.18 J/(g·ºC).
When 1.0 x 105 joules are absorbed by a piece of aluminum, the temperature of the aluminum increases from 100 ºC to 250 ºC. What is the mass of piece of aluminum? The specific heat of aluminum is 0.897 J/(g·ºC).
Ice has a specific heat of 2.06 J/(g·ºC). If 1133 joules are given off by a 50 gram piece of ice that has a temperature of -10 ºC, what is the final temperature of the piece of ice?
Iron has a specific heat of 0.449 J/(g·ºC). If 1400 joules are absorbed a chunk of iron that weighs 40 grams, how much does the temperature of the iron increase?
The molar heat of fusion for water is 6.009 kJ/mol. How much energy is required to melt 3.00 moles of ice at 0 ºC?
The molar heat of fusion for water is 6.009 kJ/mol. How much energy must be removed from 10.0 moles of water at 0 ºC in order to convert it to ice at 0 ºC?
The molar heat of vaporization for water is 40.79 kJ/mol. How much energy must be absorbed by 25 moles of water at 100 ºC in order to convert it to steam at 100 ºC?
The molar heat of vaporization for water is 40.79 kJ/mol. How much energy must be removed from 4.75 moles of steam at 100 ºC in order to condense it to water at 100 ºC?
The molar heat of vaporization for water is 40.79 kJ/mol. How much energy must be absorbed by 100 grams of water at 100 ºC in order to convert it to steam at 100 ºC?
The molar heat of fusion for water is 6.009 kJ/mol. How much energy must be absorbed by 55 grams of ice at 0 ºC in order to convert it to water at 0 ºC?
Equal masses of each of the following substances absorb an equal amount of energy. Which substance experiences the greatest temperature increase?