College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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- 100-gram oil at 20°C and 50-gram iron at 75 °C are placed in 200-gram iron container. The increase in temperature of the container is 5°C and the specific heat of oil is 0.43 cal/g °C. What is the specific heat of the iron?arrow_forwardJake pours 350 g of water at 41°C into a 750 g aluminum container that is at an initial temperature of 12°C. The specific heat of aluminum is 900 J/kg K, and that of water is 4186 J/kg K. What is the final temperature of the system, assuming no heat is exchanged with the surroundings? Group of answer choices 13°C 18 °C 32 °C 41°Carrow_forwardHow much heat is required to convert 200 grams of -25 °C ice into 150 °C steam? Useful information:Specific heat of ice = 2.06 J/g°C Specific heat of water = 4.19 J/g°CSpecific heat of steam = 2.03 J/g°CHeat of fusion of water ΔHf = 334 J/gMelting point of water = 0 °C Heat of vaporization of water ΔHv = 2257 J/gBoiling point of water = 100 °Carrow_forward
- After 28,450 J of heat are added to 500 g of ice at -20 degrees C, how much of the ice melts? Specific heat of ice is 2.01 x 103 J/kgk, and the latent heat of fusion is 334 x 103 J/kg. none of the ice 350 grams 475 grams all of the ice 25 gramsarrow_forwardA quantity of steam (350 g) at 114°C is condensed, and the resulting water is frozen into ice at 0°C. How much heat was removed? kcal =arrow_forwardWhen 22.2 grams of ice at - 20°C have absorbed 2500 calories of heat, what is the temperature of the resulting water? specific heat of ice = 0.50 cal/g °C specific heat of water = 1.0 cal/g °c latent heat of fusion = 80 cal /garrow_forward
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