1. In construction of bridges and skyscrapers, gaps must be left between adjoining steel beams to allow for the expansion and contraction of the metal due to heating and cooling. The temperature of a sample of iron with a mass of 10.0g changed from 50.4C to 25.0C with the release of 114J heat. What is the specific heat of iron? 2. If the temperature of 34.4 g of ethanol increases from 25.0C to 78.8C, how much heat has been absorbed by the ethanol? 3. A 4.50g nugget of pure gold absorbed 276 J of heat. What was the final temperature of the gold if the initial temperature was 25.0C? The specific heat of gold is 0.129J/(gC). 4. A 155g sample of an unknown substance was heated from 25.0C to 40.0C. In the process, the substance absorbed 5696J of energy. What is the specific heat of the substance? Identify the substance among those listed in Table above. 5. One lawn chair is made of aluminum and another is made of iron. Both chairs are painted the same color and have the same mass. On a sunny day, which chair will be hottest to sit in? Explain why. 6. What is the specific heat of an unknown substance if a 2.50g sample releases 12.0 J as its temperature changes from 25.0C to 20.0C? 7. A piece of metal with a mass of 4.68g absorbs 256J of heat when its temperature increase by 182C. What is the specific heat of the metal? Identify the type of metal. 8. If 335g water at 65.5C loses 9750 J of heat, what is the final temperature of the water? 9. The temperature of a sample of water increases from 20.0C to 46.6C as it absorbs 5650J of heat. What is the mass of the sample? 10. How many joules of heat are lost by 3580 kg granite as it cools from 41.2C to -12.9C? 11. How much heat is absorbed by a 2000 kg granite boulder as energy from the sun causes its temperature to change from 10C to 29C? 12. How is the quantity of heat lost by the system related to the quantity of heat gained by the surroundings during an exothermic process?