A 124 gram ice cube at -33°C is placed into a 2.50 kg iron container (assume no energy is transfered as heat to or from the surroundings). The temperature of the iron container drops by 55°C. Calculate the final temperature in °C of the water in the container. The density of water is 1.00g/mL and the heat capacity of ice to be 37.7 J mol-1K-1 and the heat capacity of water is 75.3 J mol-1K-1. The molar enthalpy of fusion of water is 6.01 kJ/mol and the heat capacity of iron is 0.45 J/(gK).

Chemistry: An Atoms First Approach
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Author:Steven S. Zumdahl, Susan A. Zumdahl
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Chapter7: Chemical Energy
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A 124 gram ice cube at -33°C is placed into a 2.50 kg iron container (assume no energy is transfered as heat to or from the surroundings). The temperature of the iron container drops by 55°C. Calculate the final temperature in °C of the water in the container. The density of water is 1.00g/mL and the heat capacity of ice to be 37.7 J mol-1K-1 and the heat capacity of water is 75.3 J mol-1K-1. The molar enthalpy of fusion of water is 6.01 kJ/mol and the heat capacity of iron is 0.45 J/(gK).

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