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Consider liquid water (sm = 69.91 JK-1mol-1) and ice (sm = 37.99 JK-1mol-1) in equilibrium at 0oc and 1 bar pressure. Calculate the difference in molar Gibbs energies of the two phases when the temperature is increased to 1oc.
Accepted Answer
Sure, here is the calculation of the difference in molar Gibbs energies of liquid water and ice when the temperature is increased from 0°C to 1°C:
$Delta G_m = Delta H_m - T Delta S_m $
$Delta H_m = 6.01 kJ/mol $
$Delta S_m = (37.99 - 69.91) J/mol K = -31.92 J/mol K $
$Delta G_m = 6010 J/mol - (273.15 K * (-31.92 J/mol K)) $
$Delta G_m = 6010 J/mol + 8733 J/mol $
$Delta G_m = 14743 J/mol $
$Delta G_m = 14.74 kJ/mol $
Therefore, the difference in molar Gibbs energies of liquid water and ice when the temperature is increased from 0°C to 1°C is 14.74 kJ/mol.
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