Spontaneous Processes (Irreversible Process)

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?

Unit of entropy is:

The Nernst equation for the reaction, ${\mathrm{A}}^{2+}+ 2{\mathrm{e}}^{-}\to \mathrm{A}$, in terms of the free energy change is:

The equilibrium concentrations of the species in the reaction $\mathrm{A}+\mathrm{B}\leftrightharpoons \mathrm{C}+\mathrm{D}$ are $2,3,10 \mathrm{and} 6 \mathrm{mol} {\mathrm{L}}^{-1}$ respectively at $300\mathrm{K}$. $∆{\mathrm{G}}^{\circ }$ for the reaction is 

$\left(\mathrm{R} =2 \mathrm{cal}/\mathrm{mol} \mathrm{K}\right)$

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)

The entropy and enthalpy changes for the process ${\mathrm{C}}_{\left(\mathrm{graphite}\right)}+{\mathrm{CO}}_2\left(\mathrm{g}\right)\to 2\mathrm{CO}\left(\mathrm{g}\right) \mathrm{are} 170 {\mathrm{JK}}^{-1} \mathrm{and} 170 \mathrm{kJ}$. At what temperature this reaction occurs spontaneously?

The spontaneity means, having the potential to proceed without the assistance of external agency. The process which occurs spontaneously are:

Standard enthalpy and standard entropy changes in a certain process at ${27}^{\mathrm{o}}\mathrm{C}$ are $-382 \mathrm{kJ}$ and $-146 {\mathrm{JK}}^{-1}$ respectively. Standard gibbs energy change of this process is:

The molar entropies of $\mathrm{HI}\left(\mathrm{g}\right),\mathrm{H}\left(\mathrm{g}\right) \mathrm{and} \mathrm{I}\left(\mathrm{g}\right)$ at $298\mathrm{K}$ are $206.5,114.6, \mathrm{and} 180.7 \mathrm{J} {\mathrm{mole}}^{\mathbf{-}\mathbf{1}} {\mathrm{K}}^{-1}$ respectively. Using the ${\mathrm{\Delta G}}^{\mathrm{o}}$ given below, The bond energy of $\mathrm{HI}$ is $\frac{\mathrm{x}}{4}\times {10}^5\mathrm{J}$. Find out the value of $\mathrm{x}$.

$\mathrm{HI}\left(\mathrm{g}\right) \to \mathrm{H}\left(\mathrm{g}\right) + \mathrm{I}\left(\mathrm{g}\right); {\mathrm{\Delta G}}^{\mathrm{o}} = 271.8 \mathrm{kJ}$

Calculate the temperature above which the reduction of lead oxide to lead in the following reaction becomes spontaneous.

$\mathrm{PbO}\left(\mathrm{s}\right)+\mathrm{C}\left(\mathrm{s}\right)\to \mathrm{Pb}\left(\mathrm{s}\right)+\mathrm{CO}\left(\mathrm{g}\right)$

$\left[\mathrm{Given}: ∆\mathrm{H} = 108.4 \mathrm{kJ} {\mathrm{mol}}^{-1}; ∆\mathrm{S} = 190 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}\right]$