Chap 5 correction - Example: Find the ∆E of H2O(l) H2O(g)...

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Unformatted text preview: Example: Find the ∆E of H2O(l) H2O(g) at 298 K and 1 atm, given ∆H = 44.0 kJ. • • • ∆E + P∆V = ∆H ∆H 1 mole of gas is produced per mole of the liquid. System expanded. w = negative Since V of liquid is negligible compared to the gas, ∆V = volume of 1 mole of gas w= - P∆V = -nRT = -1.00 mole × 8.314 J/mole⋅K × 298 K J/mole = -2478 J per = -2.48 kJ per mole of liquid vaporized ∆H = 44.0 kJ/mole = ∆E + P∆V ∆E ∆E = 44.0 + (-2.48) ∆E ∆E ∆E = 41.5 kJ 41.5 (∆E (∆E is about 5.7% less than ∆H.) less ...
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This note was uploaded on 07/30/2011 for the course CHEM 210 taught by Professor Zhang during the Spring '09 term at Shanghai Jiao Tong University.

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