What will be the value of $\Delta G$ for the melting of ice at $283 \ K$?

The values of $\Delta H$ and $\Delta S$ for the reaction,$C_{(graphite)} + CO_{2(g)} \rightarrow 2CO_{(g)}$ are $170 \ kJ$ and $170 \ J \ K^{-1}$ respectively. This reaction will be spontaneous at temperatures greater than ............ $K$.

$A$ 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.

Calculate $\Delta H^{\circ}$ for a reaction at $298 \ K$ if $\Delta S^{\circ} = 120 \ J \ K^{-1}$ and $\Delta G^{\circ} = 28000 \ J$. (in $kJ$)

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

When enthalpy and entropy change for a chemical reaction are $-2.5 \times 10^3 \ cal$ and $7.4 \ cal \ K^{-1}$ respectively,predict if the reaction at $298 \ K$ is: