1. Exercise 1 (exercise 1 p. 249) What is the specific heat of iron if 186 J of heat is required to raise the temperature of 165 g of iron from 23.2°C to 25.7°C? Solution

2. Exercise 2 (exercise 4 p. 249) If 25.00 g of metal at 90°C is placed in 50 g of water at 25°C the temperature raises to 29.8°C. (a)How much heat did the water absorb from the metal (b) What is the specific heat of the metal? Data: Specific heat of water is 4.184 J/g.°C Solution

4. Exercise 4 (exercise 3 p. 252) If 0.20 g of H 2 (g) and 1.60g of O 2 (g) react completely to give water, liberates 28.2 kJ of heat. Calculate the heat of formation of water? Solution

5. Exercise 5 (exercise 6 p. 253) When 1.2 g C(graphite) was burnt completely in sufficient oxygen gas to give CO 2 (g) and, 39.35 kJ of heat were liberated (released). Calculate the enthalpy change of formation of CO 2 under the same condition? Solution

9. Exercise 9 (exercise 1 p. 271) Determine the amount of work, in joules, done when a system consisting of 1.0 cm 3 of liquid water at 0°C freezes under a constant pressure of 1.0 atm (101. 325 kPa) and forms 1.1 cm 3 of ice. Solution

10. Exercise 10 (exercise 3 p. 271) If 600J of heat is added to a system with an internal energy E 1 and the system does 450J of work on the surrounding. (a)What is the energy change in the system ? (b) What energy change do the surrounding undergo? Solution