College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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A 0.1 kg chunk of ice at 0 C is added to 0.5 kg of water at 80 C. Assuming no heat is lost to the surroundings, what is the temperature when thermal equilibrium is reached? ( The specific heat of ice is 2090 J/(kg K), the specific heat of water is 4186 J/(kg K), and the latent heat of fusion of water is 334 kJ/kg.)
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- A 20-g ice cube floats in 180 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 90°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C, respectively.)arrow_forwardAn aluminum container whose mass is 205 g contains 300 g of water at 200C. In this container is then placed 250 g of iron at 1500C and 20 g of ice at −100C. Find the final temperature of the mixture. The specific heat of aluminum and iron is 0.21 cal/g C0 and 0.11 cal/g C0, respectively. The specific heat of ice is 0.50 cal/g C0 while its heat of fusion is 80 cal/g (handwritten please)arrow_forwardThe initial temperature of 60 g of ice is -200C. The specific heat capacity of ice is 0.5 cal/g.C0 and water’s is 1 cal/g.C0. The latent heat of fusion of water is 80 cal/g. How much heat is required to raise the ice to 00C and completely melt the ice? (b) How much additional heat is required to heat the water (obtained by melting the ice) to 620C?arrow_forward
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