?A block of copper \(\left(C_{p, \mathrm{m}}=24.44 \ \mathrm{J} \mathrm{K}^{-1} \

Chapter 3, Problem P3B.8

(choose chapter or problem)

A block of copper \(\left(C_{p, \mathrm{m}}=24.44 \ \mathrm{J} \mathrm{K}^{-1} \ \mathrm{mol}^{-1}\right)\) of mass 2.00 kg and at \(0^{\circ} \mathrm{C}\) is introduced into an insulated container in which there is \(1.00\mathrm{mol} \ \mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) at \(100^{\circ} \mathrm{C}\) 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.

Text Transcription:

(C_p,m = 24.44 J K^−1 mol^−1)

0 degree C

100 degree C

1.00molH_2O(g)