A block of copper (Cp,m = 24.44 J K−1 mol−1) of mass 2.00 kg and at 0 °C is introduced into an insulated container in which there is 1.00 mol H2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed to liquid water, determine: (a) the final temperature of the system; (b) the heat transferred to the copper block; and (c) the entropy change of the water, the copper block, and the total system. The data needed are given in Exercise E3B.7a.

A block of copper (Cp,m = 24.44 J K−1 mol−1) of mass 2.00 kg and at 0 °C is introduced into an insulated container in which there is 1.00 mol H2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed to liquid water, determine: (a) the final temperature of the system; (b) the heat transferred to the copper block; and (c) the entropy change of the water, the copper block, and the total system. The data needed are given in Exercise E3B.7a.

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Question

A block of copper (C_p,m = 24.44 J K⁻¹ mol⁻¹) of mass 2.00 kg and at 0 °C is introduced into an insulated container in which there is 1.00 mol H2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed to liquid water, determine: (a) the final temperature of the system; (b) the heat transferred to the copper block; and (c) the entropy change of the water, the copper block, and the total system. The data needed are given in Exercise E3B.7a.

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