1. 1)A 32.07 g sample of vanadium (specific heat of 0.49 J/g˚C) was heated to 75.00 ˚C (its initial temperature). This piece of vanadium is then placed into 100.0 g of water with an initial temperature of 22.50 ˚C and a specific heat of 4.18 J/g ˚C. The metal and water are allowed to come to thermal equilibrium. What is the final temperature of the water and metal?

2. 2) A piece of unknown metal was a mass of 17.19 g is heated to an initial temperature of 92.5 ˚C and placed into 25.00 g of water at an initial temperature of 24.50 ˚C. The final temperature of the system is 30.05 ˚C. What is the specific heat of the metal when the specific heat of the water is 4.18 J/g ˚C.

3. 3) A piece of rhodium with a mass of 24.5 g, a specific heat of 0.242 J/g˚C, and an initial temperature of 90.0 ˚C is added to 30.08 g of water, whose specific heat is 4.18 J/g˚C. The final temperature of the metal and water was 30.7 ˚C. What was the initial temperature of the water?

4. 4) 125 g of water has an initial temperature of 35 ˚C, and a specific heat of 4.18 J/g ˚C. After being mixed with a piece of silver, with a specific heat of 0.240 J/g ˚C and initial temperature of 130.0 ˚C, the water and silver have a final temperature of 60.0 ˚C. What was the mass of the piece of silver?

5. 5) A 30.5 g sample of nickel, with a specific heat of 0.440 J/g ˚C and an initial temperature of 230 ˚C, is added to water at an initial temperature of 50. ˚C and a specific heat of 4.18 J/g ˚C. The final temperature of the nickel and water is 135 ˚C. What mass of water was the nickel added to?

6. 6) A 55.0 g sample of water is heated to an initial temperature of 95.3 ˚C. A 32.79g cooled sample of copper metal is placed in the water and the copper and metal are allowed to come to thermal equilibrium. The final temperature of the copper and water is 71.8 ˚C. What was the initial temperature of the copper given the specific heat of water at 4.18 J/g ˚C and the specific heat of copper is 0.385 J/g ˚C.