Problem Solving

1. Convert the following quantities.

a. 46^oC to K b. 467 K to ^oC c. - 57^oC to K d. 268 K to ^oC

2. Calculate the energy required to heat 10.4 g of mercury form 37.0^oC to 42.0^oC. The specific heat of mercury is 0.14 J/g^oC.

3. A total of 50 J of heat are applied to 10 g of iron. If the initial temperature of the iron is room temperature (22^oC), what is the final temperature of the sample of iron if its heat capacity is 0.45 J/g^oC.

4. A 10 g sample of aluminum, with a specific heat capacity of 0.90 J/g^oC, has an initial temperature of 22^oC. If 300 J of heat is added to the sample, what is its final temperature?

5. What mass of water will change its temperature by 3oC when 525 J of heat is added to it? The specific heat capacity of water is 4.18 J/g^oC.

The following questions will involve phase changes. Please make sure account for, when applicable, the Latent heat of fusion and Vaporization.

6. How many joules are required to heat 200 g of water from 25^oC to 125^oC? The specific heat capacity of water is 4.18 J/g^oC.

7. How many joules are required to heat 75 g of water from - 85^oC to 185^oC?

8. How many joules are required to heat a frozen can of juice (360 g) from - 5^oC (the temperature of an overcooled refrigerator) to 110^oC (the highest practical temperature within a microwave oven)?