?Consider a process in which \(1.00 \mathrm{mol} \ \mathrm{H}_{2}

Chapter 3, Problem P3B.1

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Consider a process in which \(1.00 \mathrm{mol} \ \mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) at \(-5.0 \ ^{\circ} \mathrm{C}\) solidifies to ice at the same temperature. Calculate the change in the entropy of the sample, of the surroundings and the total change in the entropy. Is the process spontaneous? Repeat the calculation for a process in which \(1.00 \mathrm{mol} \ \mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) vaporizes at \(95.0 \ ^{\circ} \mathrm{C}\) and 1.00 atm. The data required are given in Exercise E3B.7(a).

Text Transcription:

-5.0 degree C

95.0 degree C

1.00molH_wO(l)

1.00molH_wO(l)

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