The standard enthalpy and standard entropy of decomposition of $N_2O_4$ to $NO_2$ are $55.0 \ kJ \ mol^{-1}$ and $175.0 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard free energy change for this reaction at $25 ^{\circ}C$ in $J \ mol^{-1}$ is $............$ $(Nearest \ integer)$.

The densities of graphite and diamond at $298 \, K$ are $2.25 \, g \, cm^{-3}$ and $3.31 \, g \, cm^{-3}$ respectively. If the standard free energy difference $(\Delta G^o)$ is $1895 \, J \, mol^{-1}$, the pressure at which graphite will be transformed into diamond at $298 \, K$ is:

The standard reaction Gibbs energy for a chemical reaction at an absolute temperature $T$ is given by $\Delta_{r}G^{o} = A - BT$,where $A$ and $B$ are non-$zero$ constants. Which of the following is $TRUE$ about this reaction?

The reaction $MgO_{(s)} + C_{(s)} \to Mg_{(s)} + CO_{(g)}$,for which $\Delta_r H^o = +491.1 \ kJ \ mol^{-1}$ and $\Delta_r S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$,is not feasible at $298 \ K$. The temperature above which the reaction will be feasible is ..... $K$.

$A$ process will be spontaneous at all temperatures if

Consider the graph of $Gibbs$ free energy $G$ vs. Extent of reaction. The number of statement$(s)$ from the following which are true with respect to points $(a)$,$(b)$,and $(c)$ is $.................$
$A$. Reaction is spontaneous at $(a)$ and $(b)$
$B$. Reaction is at equilibrium at point $(b)$ and non-spontaneous at point $(c)$
$C$. Reaction is spontaneous at $(a)$ and non-spontaneous at $(c)$
$D$. Reaction is non-spontaneous at $(a)$ and $(b)$