The sketch above shows the Gibbs free energy of water at 373 K as a function of

Question

The sketch above shows the Gibbs free energy of water at 373 K as a function of pressure.

A) Why is the slope of the vapor line at 0.2 bar steeper than the slope of this line at 0.7 bar?

B) Why is the slope of the vapor line steeper than the liquid line?

C) At 1.1 bar, the vapor line is above the liquid line. Use this information to determine whether or not the transformation of water vapor into liquid water at 373 K and 1.1 bar is spontaneous. If you do not have enough information, explain what additional information is needed. Briefly explain your reasoning.

Explanation / Answer

at 0.2 bar ,it is in gaseous state.the entropy of gaseous state is more than liquid state.gas has more entropy than liquid molecule,so it is higher(actually (dG/dP)at const.T= V,volume-which indicating entropy

B)this is also for same reason,entropy of vapour is more than liquid

C)(dG/dP)at const. Temp(373K) = V of water.at that pressure if dG=o,then transformation can occure

condition for phase tranformation is dG=0,at that point tangent of both curve =0 ,then it is possible(for fixed mass)

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