A 1.00 -kg gold bar is taken from a forge at 800 degrees * C and dropped into 4.00 kg of water at 10.0 °C . Assuming that no energy is lost by heat to the surroundings , determine the total entropy change of the bar-plus- water system.
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A 1.00 -kg gold bar is taken from a forge at 800 degrees * C and dropped into 4.00 kg of water at 10.0 °C . Assuming that no energy is lost by heat to the surroundings , determine the total entropy change of the bar-plus- water system.
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- A 0.50-kg piece of aluminum at 250 °C is dropped into 1.0 kg of water at 20 °C . After equilibrium is reached, what is the net entropy change of the system?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/KCalculate the change in entropy as 0.3989 kg of ice at 273.15 K melts. The latent heat of fusion of water is 333000 J/kg.