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Standard Gibbs energy of reaction (Delta_(r)G^(@)) at a certain temperature can be completed as Delta_(r)G^(@)=Delta_(r)H^(@)-Tdelta_(r)S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows: Delta _(r) H_(T_(2))^(@)-Delta_(r)C_(p)^(@)(T_(2)-T_(1)) Delta_(r)S_(T_(2))^(@)-Delta_(r)S_(T_(1))^(@)=Delta_(r)C_(p)^(@)In ((T_(2))/(T_(2))) Delta_(r)G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) Delta_(r)^(@)G^(@)=-RTInK_(eq) Consider the following reaction : CO(g)+2H_(2)(g)toCH_(3)OH(g) Given Delta_(r)H^(@)(CH_(3)Oh,g]=-201KJ//mol Delta_(r)H^(@)(CO,g)=-114KJ//mol s^(@)(CH_(3)OH,g)=240J//mol-k, S^(@)(H_(2)g)=198J//mol-KC_(p.m)^(@)(h_(2))=28.8JK^(-1)mol^(-1) C_(p.m(CO)=29.4J//mol-K C_(p.m)^(@)(CH_(3_)OH)=44J//mol-K and In ((320)/(300))=0.06,"all data at"300K. Delta_(r)s^(@)at 320K is: |
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Answer» 155.18 J/mol-K |
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