The standard enthalpy of the decomposition of $N_2O_4$ to $NO_2$ is $58.04 \, kJ$ and standard entropy of this reaction is $176.7 \, J/K$. The standard free energy change for this reaction at $25 \, ^oC$ is $..... \, kJ$

The free energy for a reaction having $\Delta H = 31400 \, cal$ and $\Delta S = 32 \, cal \, K^{-1} \, mol^{-1}$ at $1000 \, ^oC$ is ....... $cal$.

$A$ reaction,$A + B \rightarrow C + D + q$,is found to have a positive entropy change. The reaction will be:

The signs of $\Delta_r H^{\circ}$ and $\Delta_r S^{\circ}$ for a reaction to be spontaneous at all temperatures respectively are

The values of $\Delta H$ and $\Delta S$ of a certain reaction are $-400 \text{ kJ mol}^{-1}$ and $-20 \text{ kJ mol}^{-1} \text{ K}^{-1}$ respectively. The temperature below which the reaction is spontaneous, is

The maximum work (in $kJ \, mol^{-1}$) that can be derived from the complete combustion of $1 \, mole$ of $CO$ at $298 \, K$ and $1 \, atm$ is:
[Standard enthalpy of combustion of $CO = -283.0 \, kJ \, mol^{-1}$; standard molar entropies: $S_{O_2} = 205.1 \, J \, K^{-1} \, mol^{-1}$,$S_{CO} = 197.7 \, J \, K^{-1} \, mol^{-1}$,$S_{CO_2} = 213.7 \, J \, K^{-1} \, mol^{-1}$]