A sample of 1.0 molgaseous water is condensed isothermally and reversibly to liq

Question

A sample of 1.0 molgaseous water is condensed isothermally and reversibly to liquidwater at 100 C. The standard enthalpy of vaporization of water at100 C is 40.656 kJ/mol. Find the internal energy change for thisthermodynamic process. A sample of 1.0 molgaseous water is condensed isothermally and reversibly to liquidwater at 100 C. The standard enthalpy of vaporization of water at100 C is 40.656 kJ/mol. Find the internal energy change for thisthermodynamic process. 54.33kJ -37.55kJ -27.74kJ +38.34kJ

Explanation / Answer

   1H2O (g) ...........>1H2O (l) Formula : H = U + nRT n = number of moles of gaseous products -   number of moles of gaseous reactants        = 0 - 1        = -1 Given , H = 40.656kJ/mol        -40.656kJ =U + (-1mol)(8.314J.mol-1.K-1)(393K)           -40.656kJ = U   - 3.2674kJ                         U = -40.656kJ +  3.2674kJ                                 =-37.40 kJ Second option is correct. Second option is correct.

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