For a chemical reaction,if $\Delta H = \Delta S > 0$,then $\Delta H = $ ................

For the given reaction: $H_{2(g)} + S_{(s)} \to H_2S_{(g)}$; $\Delta H_r = 100\, kJ/mol$ and $\Delta S_r = 400\, J/mol\cdot K$. The temperature at which the above reaction occurs reversibly is (Assuming $\Delta H_r$ and $\Delta S_r$ are independent of temperature) ..... $K$.

At the transition temperature $T$,$\Delta G^0 = 0$ and $\Delta G^0 = 105 - 35 \log T$,where $A$ and $B$ are two states of substance $X$. The transition temperature in $^\circ\text{C}$ when pressure is $1 \text{ atm}$ is . . . . . . .

If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

The value of ${\left[ {\frac{dG}{dT}} \right]_P}$ is ....

$A$ spontaneous process is impossible if ........