How much thermal energy is required to boil 2.0 kg of water at into steam at The latent heat of vaporization of water is and the specific heat of steam is
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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.
What mass (in grams) of steam at 100°C must be mixed with 298 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 15.0°C? The specific heat of water is 4186 J/kg·K. The latent heat of fusion is 333 kJ/kg, and the latent heat of vaporization is 2256 kJ/kg.
