Answer
$\Delta_{r}G^{\circ}=28.63\,kJ/mol$
The reaction is reactant-favored.
Work Step by Step
$\Delta_{r}G^{\circ}=\Delta _{r}H^{\circ}-T\Delta _{r}S^{\circ}$
$=41.17\,kJ/mol-(25+273)K(42.08\,JK^{-1}mol^{-1})$
$=41.17\,kJ/mol-(298\,K)(0.04208\,kJK^{-1}mol^{-1})$
$=28.63\,kJ/mol$
$\Delta_{r}G^{\circ}$ is positive.
$\implies$ The reaction is reactant-favored.
