The surface of the Sun is approximately 5,550 K, and the temperature of the Earth's surface is approximately 289 K. What entropy change occurs when 5,000 J of energy is transferred by heat from the Sun to the Earth? (J/K)
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The surface of the Sun is approximately 5,550 K, and the temperature of the Earth's surface is approximately 289 K. What entropy change occurs when 5,000 J of energy is transferred by heat from the Sun to the Earth? (J/K)
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- A heat source generates heat at a rate of 63.0 W (1 W=1 J/s). How much entropy does this produce per hour in the surroundings at 27.2 ∘C Assume the heat transfer is reversible.What is the decrease in entropy of 44.8 g of water that condenses on a bathroom mirror at a temperature of 39.7°C, assuming no change in temperature and given the latent heat of vaporization to be 2450 kJ/kg? Select the correct answer O 396 J/K O 189 J/K X Your Answer O 209 J/K 351 J/K O 251 J/KHow much energy must be transferred as heat for a reversible isothermal expansion of an ideal gas at 132°C if the entropy of the gas increases by 46.0 K
- A Styrofoam cup holding 118 g of hot water at 1.00 x 10-°C cools to room temperature, 21.0°C. What is the change in entropy of the room? (Neglect the specific heat of the cup and any change in temperature of the room. The specific heat of water is 4,186 J/(kg · °C).) J/KA Styrofoam cup holding 142 g of hot water at 1.00 ✕ 102°C cools to room temperature, 21.0°C. What is the change in entropy of the room? (Neglect the specific heat of the cup and any change in temperature of the room. The specific heat of water is 4,186 J/(kg · °C).)__________ J/KCalculate the entropy of rolling a die three times such that the sum of numbers for the first two observations is divisible by the number obtained third time. (a) 6.47 x103 J/K (b) 2.03 m -kg-s.K (c) 2.81 m² - kg -s. K (d) 2.81x10-3 J/K
- What is the decrease in entropy (in J/K) of 30.0 g of water that condenses on a bathroom mirror at a temperature of 33.5°C, assuming no change in temperature and given the latent heat of vaporization to be 2450 kJ/kg?A room is at a constant 295 K maintained by an air conditioner that pumps heat out. How much does the refrigerator change the entropy AS of the room for each 5.80 kJ of heat that it removes? AS = J/KA 100-lbm block of a solid material whose specific heat is 0.5 Btu/lbm·R is at 80°F. It is heated with 10 lbm of saturated water vapor that has a constant pressure of 20 psia. Determine the final temperature of the block and water, and the entropy change of the entire system. Is this process possible? Why?