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-K``C_(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)H^(@) `at 300K for the reaction is :A. `-87KJ/mol`B. `87KJ//mol`C. `172J//mol-K`D. none of these