A 200 g copper bowl contains 190 g of water, both at 22.0°C. A very hot 380 g copper cylinder is dropped into the water, causing the water to boil, with 17.0 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature 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 200 g copper bowl contains 190 g of water, both at 22.0°C. A very hot 380 g copper cylinder is dropped into the water, causing the water to boil, with 17.0 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature 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.

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Question

A 200 g copper bowl contains 190 g of water, both at 22.0°C. A very hot 380 g copper cylinder is dropped into the water, causing the water to boil, with 17.0 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature 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.

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