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27 Nov 2019
A 190 g copper bowl contains 180 g of water, both at 23.0°C. A very hot 450 g copper cylinder is dropped into the water, causing the water to boil, with 6.37 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature (in Celsius) of the cylinder? The specific heat of water is 1 cal/g·K, and of copper is 0.0923 cal/g·K. The latent heat of vaporization of water is 539 Cal/kg.
A 190 g copper bowl contains 180 g of water, both at 23.0°C. A very hot 450 g copper cylinder is dropped into the water, causing the water to boil, with 6.37 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature (in Celsius) of the cylinder? The specific heat of water is 1 cal/g·K, and of copper is 0.0923 cal/g·K. The latent heat of vaporization of water is 539 Cal/kg.
