For a spontaneous change,free energy change $\Delta G$ is

Calculate the work done (in $J$) when $4.5 \ g$ of $H_2O_2$ reacts against a pressure of $1.0 \ atm$ at $25 \ ^oC$. [$2H_2O_{2(l)} \to O_{2(g)} + 2H_2O_{(l)}$]

Calculate the value of $\Delta G$ for the following reaction: $N_2O_{4(g)} \longrightarrow 2NO_{2(g)}$ if $\Delta H = 57.44 \ kJ$ and $\Delta S = 176 \ J \ K^{-1} \ mol^{-1}$ at $300 \ K$. (in $kJ$)

Under what conditions will a reaction become spontaneous at all temperatures?

$A$ reaction has both $\Delta H$ and $\Delta S$ negative. The rate of reaction

$A$ process has $\Delta H = 200 \ J \ mol^{-1}$ and $\Delta S = 40 \ J \ K^{-1} \ mol^{-1}$. Choose the minimum temperature above which the process will be spontaneous.