CALORIMETRY WORKSHEET #2
SOLVE THESE PROBLEMS ON A SEPARATE SHEET OF PAPER. SHOW ALL WORK. INCLUDE
UNITS DURING YOUR SETUP OF THE PROBLEM. USE SIGNIFICANT FIGURES FOR ALL
PROBLEMS.
The specific heat of water, 1 cal/g°C or 4.184 J/g°C are defined values and do NOT affect significant
figures. These problems are a review of using the specific heat equation.
1.
Calculate the energy needed to raise the temperature of 25.0 grams of water from 22.0°C to 31.0°C.
Use calories.
2.
Calculate the energy needed to raise the temperature of 177.2 grams of water from 27.8°C to 45.7°C.
Use joules.
3.
Calculate the energy lost when 73.5 grams of water goes from 87.5°C to 60.5°C.
Use calories.
4.
Calculate the energy lost when 9.20 grams of water goes from 54.3°C to 21.2°C.
Use joules.
Energy can not be created nor destroyed. For problems 5-8, set the energy lost by the metal equal to the
energy gained by the water and solve for the missing variable. IN OTHER WORDS, YOU NEED TO
HAVE TWO PARTS TO YOUR EQUATION BECAUSE THERE ARE TWO SUBSTANCES THAT
ARE UNDERGOING HEAT ENERGY CHANGES. DRAW A PICTURE TO HELP!
5.
A piece of lead is heated to a temperature of 91.0 °C and placed in 125 grams of water at 25.0 °C. The
final temperature of the water and metal is 31.5 °C. The specific heat of lead is 0.160 J/g °C. What is
the mass of the piece of lead?
6.
30.0 grams of a metal sample at a temperature of 122°C are placed in 80.0 grams of water at a
temperature of 15.0°C. The final temperature of the water and metal is 21.5°C. What is the specific heat
of the metal?
7.
40.0 grams of aluminum at a temperature of 180.°C are placed in 250. grams of water at 22.0°C. The
specific heat of the aluminum is 0.22 cal/g°C. What is the final temperature of the water and metal? The
specific heat of water is 1 cal/g°C.
8.
45.0 grams of a metal sample at a temperature of 121°C are placed in 75.0 grams of water at a
temperature of 25.0°C. The final temperature of the water and metal is 29.3°C. What is the specific heat
of the metal in units of J/g°C?