Gibbs Energy Change and Equilibrium

Match list-I (Equations) with List-II (Type of processes) and select the correct option.
 

Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?

For the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2{\mathrm{NH}}_3\left(\mathrm{g}\right);∆\mathrm{H}=-99.4\mathrm{kJ}$ and $∆\mathrm{S}=-198.3{\mathrm{JK}}^{-1}$. The temperature at which the system is in equilibrium is

For the reaction at $298 \mathrm{K} 2 \mathrm{A}+\mathrm{B}=\mathrm{C}$
$\mathrm{\Delta H}=40{\mathrm{kJmol}}^{-1}$ and $\mathrm{\Delta S}=0.02 {\mathrm{kJmol}}^{-1}{\mathrm{K}}^{-1}$. At what temperature will the reaction becomes spontaneous considering $\mathrm{\Delta H}$ and $\mathrm{\Delta S}$ to be constant over the temperature range,

If $∆\mathrm{G}$ for a reaction is negative, the change is:

The maximum work (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$) that can be derived from complete combustion of $1$ mole of $\mathrm{CO}$ at $298 \mathrm{K}$ and $1 \mathrm{atm}$ is [Standard enthalpy of combustion of $\mathrm{CO}=-283.0 \mathrm{kJ} {\mathrm{mol}}^{-1}$; standard molar entropies at $298 \mathrm{K}: {\mathrm{S}}_{{\mathrm{O}}_2}=205.1 \mathrm{J} {\mathrm{mol}}^{-1}, {\mathrm{S}}_{\mathrm{CO}}=197.7 \mathrm{J} {\mathrm{mol}}^{-1}. {\mathrm{S}}_{{\mathrm{CO}}_2}=213.7 \mathrm{J} {\mathrm{mol}}^{-1}$]

Which condition among the following holds true at the stage of half-completion for the reaction $\mathrm{A}\rightleftharpoons \mathrm{B} ?$

The boiling point of water at $1 \mathrm{atm}$ is $100°\mathrm{C}.$ Which among the following is true for vaporization of water at $75°\mathrm{C} ?$

For the process

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\left(1\mathrm{ }\mathrm{b}\mathrm{a}\mathrm{r},\mathrm{ }373\mathrm{ }\mathrm{K}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)(1\mathrm{ }\mathrm{b}\mathrm{a}\mathrm{r},\mathrm{ }373\mathrm{ }\mathrm{K})$ , the correct set of thermodynamic parameters is

A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following:

For the reaction $2{\mathrm{O}}_3\to 3{\mathrm{O}}_2, \mathrm{\Delta H}, \mathrm{\Delta S}$ and $∆\mathrm{G}$ are respectively:

Assuming ideal behaviour, the magnitude of $\log \mathrm{K}$ for the following reaction at $25°\mathrm{C}$ is $\mathrm{x}\times {10}^{-1}.$ The value of $\mathrm{x}$ is____________. (Integer answer) $3\mathrm{HC}\equiv {\mathrm{CH}}_{\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{C}}_6{\mathrm{H}}_{6\left(\mathrm{l}\right)}$ [Given : ${\mathrm{\Delta }}_{\mathrm{f}}\mathrm{G}°(\mathrm{HC}\equiv \mathrm{CH})=-2.04\times {10}^5] {\mathrm{mol}}^{-1}; {\mathrm{\Delta }}_{\mathrm{f}}\mathrm{G}°\left({\mathrm{C}}_6{\mathrm{H}}_6\right)=-1.24\times {10}^5 \mathrm{J} {\mathrm{mol}}^{-1}$
$\mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$]

For a dimerization reaction, $2\mathrm{A}\left(\mathrm{g}\right)\to {\mathrm{A}}_2\left(\mathrm{g}\right)$ at $298 \mathrm{K},$

${\mathrm{\Delta U}}^{\circ }=-20 \mathrm{kJ} {\mathrm{mol}}^{-1}, {\mathrm{\Delta S}}^{\circ }=-30 \mathrm{J} {\mathrm{mol}}^{-1}$, then the magnitude of ${\mathrm{\Delta G}}^{\circ }$ will be________$\mathrm{kJ}.$

Round off your answer to the nearest integer after multiplying with 2.

Products are favoured in a chemical reaction taking place at a constant temperature and pressure. Consider the following statements:
(i) The change in Gibbs energy for the reaction is negative.
(ii) The total change in Gibbs energy for the reaction and the surroundings is negative.
(iii) The change in entropy for the reaction is positive.
(iv) The total change in entropy for the reaction and the surroundings is positive.

The statements which are ALWAYS true are:-