TS EAMCET 2020 (9-Sep Shift-1)

The equilibrium constant for the reaction is ${\mathrm{P}}_4\left(\mathrm{s}\right)+{50}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{P}}_4{0}_{10}\left(\mathrm{s}\right)$

For a reaction $2{\mathrm{A}}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{B}}_{\left(\mathrm{g}\right)}+{\mathrm{C}}_{\left(\mathrm{g}\right)},{\mathrm{K}}_{\mathrm{c}}=3.75\times {10}^{-6}$ at $1069 \mathrm{K}$. The approximate value of ${\mathrm{K}}_{\mathrm{p}}$ for this reaction at the same temperature is $\left(\mathrm{R}=0.082 \mathrm{L}\right.\mathrm{bar}\left.{\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}\right)$

For the reaction ${\mathrm{A}}_{\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{B}}_{\left(\mathrm{g}\right)}+{\mathrm{C}}_{\left(\mathrm{g}\right)}, \mathrm{A}$ is $33\%$ dissociated at a total pressure $\mathrm{P}.$ The correct relation between $\mathrm{P}$ and ${\mathrm{K}}_{\mathrm{p}}$ is

The value of the reactant quotient $\left(\varnothing \right)$for the cell is
$\mathrm{Zn}\left(\mathrm{s}\right)/{\mathrm{Zn}}^{2+}\left(0.01\mathrm{M}\right)\Vert {\mathrm{Cu}}^{2+}\left(1.25\mathrm{M}\right)/\mathrm{Cu}\left(\mathrm{s}\right)$

For a reaction $2\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}, {\mathrm{K}}_{\mathrm{c}}$ is $2\times {10}^{-3}.$ At a given time, the reaction mixture has $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3\times {10}^{-4}\mathrm{M}.$ Which of the following options is correct?

Following lists contain reactions and their corresponding equilibrium constants at different temperatures:

If $∆{\mathrm{H}}_1^0 \mathrm{and} ∆{\mathrm{H}}_2^0$ are the standard enthalpies for the reactions $2{\mathrm{SO}}_2 + {\mathrm{O}}_2 \rightleftharpoons 2{\mathrm{SO}}_3 \mathrm{and} {\mathrm{N}}_2{\mathrm{O}}_4 \rightleftharpoons 2{\mathrm{NO}}_2$  respectively, then: 

The equilibrium constant $\left({\mathrm{K}}_{\mathrm{p}}\right)$ for the formation of ammonia from its constituent elements at $27°\mathrm{C}$ is $1.2\times {10}^{-4}$ and at $127°\mathrm{C}$ is $0.60\times {10}^{-4}.$ Calculate the mean heat of formation of ammonia per mole in this temperature range.

At $298 \mathrm{K}$, the equilibrium constant of the process $1.5{\mathrm{O}}_{2 \left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{O}}_{3 \left(\mathrm{g}\right)}$ is $3\times {10}^{-29}$. Standard free energy change (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$ ) of the process is approximately $\left(\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}; \log 3=0.47\right)$