Name: ______________________
Final Temp of mixed solutions of differing temperature and specific heat worksheet
1) Determine the final temperature when 45.0 g of water at 20.0 °C mixes with 22.3 grams of water at
85.0 °C.
Solution:
2) Determine the final temperature when 30.0 g of water at 8.00 °C mixes with 60.0 grams of water at
28.2 °C.
Solution:
3) Determine the final temperature when a 25.0 g piece of iron at 85.0 °C is placed into 75.0 grams of
water at 20.0 °C.
specific heat value for iron is 0.45 J per gram degree Celsius.
Solution:
4) Determine the final temperature when 10.0 g of aluminum at 130.0 °C mixes with 200.0 grams of
water at 25.0 °C.
Solution:
5) 10.0 g of water is at 59.0 °C. If 3.00 g of gold at 15.2 °C is placed in the calorimeter, what is
the final temperature of the water in the calorimeter? (The specific heat of gold is 0.128 J/g
°C.)
Solution:
6) A 29.5 g sample of methanol at 208.9 K is mixed with 54.3 g of methanol at 302.3 K. Calculate the
final temperature of the mixture assuming no heat is lost to the containers and surroundings. The
specific heat of methanol is 2.53 J g¯1 K¯1
Solution:
7) A sheet of nickel weighing 10.0 g and at a temperature of 18.0 °C is placed flat on a sheet of iron
weighing 20.0 g and at a temperature of 55.6 °C. What is the final temperature of the combined
metals? Assume that no heat is lost to the surroundings.
Specific heat nickel 0.54 J g¯1 °C¯1 and iron 0.46 J g¯1 °C¯1
Solution:
8) 105.0 mL of H2O is initially at room temperature (22.0 °C). A chilled steel rod (2.00 °C) is
placed in the water. If the final temperature of the system is 21.5 °C, what is the mass of the
steel bar? (specific heat of water = 4.184 J/g °C; specific heat of steel = 0.452 J/g °C)
Solution:
9) How many grams of water can be heated form 25.0 °C to 35.0 °C by the heat released from
85.0 g of iron that cools from 85.0 °C to 35.0 °C? The specific heat of iron is 0.450 J/g °C
Solution: