Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The Haber’s process for the formation of ${\mathrm{NH}}_3$ at $298 \mathrm{K}$ is ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3;\mathrm{\hspace{0.17em}}\mathrm{\Delta H}=-46.0\mathrm{KJ}$. Which of the following is the correct statement?

A schematic plot of ln  $K_{\mathrm{eq}}$ versus inverse of temperature for a reaction is shown below

The reaction must be –

The value of equilibrium constant for a reversible reaction is $3\times {10}^{-2}$, If the reaction quotient for the same reaction is $5\times {10}^{-3}$, predict the direction of equilibrium reaction.

In a one-litre flask, $6$ moles of $\mathrm{A}$ undergoes the reaction $\mathrm{A}( \mathrm{g})\rightleftharpoons \mathrm{P}( \mathrm{g})$. The progress of product formation at two temperatures (in Kelvin), ${\mathrm{T}}_1$ and ${\mathrm{T}}_2$, is shown in the figure:

If ${\mathrm{T}}_1=2{\mathrm{T}}_2$ and$\left({\mathrm{\Delta G}}_2^{\mathrm{o}}-{\mathrm{\Delta G}}_1^{\mathrm{o}}\right)={\mathrm{RT}}_2\mathrm{lnx}$ , then the value of $\mathrm{x}$ is
[ ${\mathrm{\Delta G}}_1^{\mathrm{o}}$ and ${\mathrm{\Delta G}}_2^{\mathrm{o}}$ are standard Gibb's free energy change for the reaction at temperatures ${\mathrm{T}}_1$ and ${\mathrm{T}}_2$, respectively.]

The value of $\log \mathrm{K}$ for the reaction $\mathrm{A}\rightleftharpoons \mathrm{B}$ at $298 \mathrm{K}$ is $\_\_\_\_\_\_\_.$ (Nearest integer)

Given: $\Delta \mathrm{H}°=-54.07 \mathrm{kJ} {\mathrm{mol}}^{-1}$

$\Delta \mathrm{S}°=10{\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$

(Taken $2.303\times 8.314\times 298=5705$ )

Derive the relationship between Equilibrium Constant (K), Reaction Quotient(q) and Gibbs Energy(G).

Give the relationship between equilibrium constant (k), reaction Quotient (Q), and Gibbs energy (G) 

For a sponatneous reaction the value of $∆{\mathrm{G}}^0$ must be negative, and the value of ${\mathrm{K}}_{\mathrm{eq}}$ must be greater than _____

(Given $∆{\mathrm{G}}^0=-\mathrm{RT} {\mathrm{lnK}}_{\mathrm{eq}}$)

What is the (approx) partial pressure of ${\mathrm{CO}}_2$at equilibrium at $427°\mathrm{C}$?

${\mathrm{CaCO}}_{3\left(\mathrm{s}\right)}\stackrel{}{\rightleftharpoons }{\mathrm{CaO}}_{\left(\mathrm{s}\right)}+{\mathrm{CO}}_{2\left(\mathrm{g}\right)} ∆{\mathrm{G}}^{\circ }=-13.5 \mathrm{kJ}$

${\mathrm{\Delta }}_{\mathrm{f}}{\mathrm{G}}^{\mathrm{o}}$ at $500 \mathrm{K}$  for substance $\text{'}\mathrm{S}\text{'}$ in liquid state and gaseous state are $+100.7 \mathrm{kcal} {\mathrm{mol}}^{-1}$ and $+103 \mathrm{kcal} {\mathrm{mol}}^{-1}$, respectively.

 Vapour pressure of liquid$\text{'}\mathrm{S}\text{'}$ at $500 \mathrm{K}$  is approximately equal to: $(\mathrm{R}=2 \mathrm{cal} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1})$.

What is the ${\mathrm{logK}}_{\mathrm{eq}}$ of the following reaction?

 $\mathrm{\Delta G}°=-0.10 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O} \left(\mathrm{s}\right)\rightleftharpoons {\mathrm{CuSO}}_4.3{\mathrm{H}}_2\mathrm{O} \left(\mathrm{s}\right)+2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right) {\mathrm{K}}_{\mathrm{p}}=0.4\times {10}^{-3} {\mathrm{atm}}^2$
Which of the following is not true for the above equilibrium?

Which of the following options will be correct for the stage of half completion of the reaction $\mathrm{A} \rightleftharpoons \mathrm{B}$?

At $60{}^{\circ }\mathrm{C}, 50\%$ of ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)$ is dissociated to ${\mathrm{NO}}_2\left(\mathrm{g}\right)$. What is the approximate standard Gibbs free energy change at $60{}^{\circ }\mathrm{C}$ and $1 \mathrm{atm}$ pressure for this process? $\left(\mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}\right)$.

The Haber’s process for the formation of ${\mathrm{NH}}_3$ at $298 \mathrm{K}$ is ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3;\mathrm{\hspace{0.17em}}\mathrm{\Delta H}=-46.0\mathrm{KJ}$. Which of the following is the correct statement?

Select the correct option about $\mathrm{\Delta G}$ for the following reaction

$\begin{array}{ccc}\underset{(2 \mathrm{atm},373 \mathrm{K})}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}& ⟶& \underset{ (2 \mathrm{atm},373 \mathrm{K})}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)}\end{array}$

(Given: $0.0821\times 373\times \ln 2=21.23 \mathrm{L} \mathrm{atm}$, molar volume of water at $2 \mathrm{atm}, 373 \mathrm{K}=18 \mathrm{ml}$)

$\mathrm{\Delta }{\mathrm{G}}^{\mathrm{o}}=+\mathrm{ }63.3\mathrm{ }\mathrm{k}\mathrm{J}$ for the reaction ${\mathrm{Ag}}_2{\mathrm{CO}}_3\left(\mathrm{s}\right)\to 2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{CO}}_3^{-2}\left(\mathrm{aq}\right)$
the thermodynamic equilibrium constant at ${25}^{\mathrm{o}}\mathrm{C}$ is:

Which of the following is correct at equilibrium?

Select the graph which can be used to determine standard free energy of the reaction given below:

${\mathrm{CaCO}}_3\left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$
Assume that the reaction is at equilibrium.

Among the following set of conditions, which condition necessarily holds true for a non-feasible process?
(Where, $\mathrm{K}=$equilibrium constant)