S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Equilibrium in Physical and Chemical Processes, Exercise 24: Competition Focus

Which of the following lines correctly show the temperature dependence of equilibrium constant $\mathrm{K}$, for an exothermic reaction?

Which of the following are reversible reactions?

Which of the following statements are wrong?

The equilibrium ${\mathrm{SO}}_2{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_2 \left(\mathrm{g}\right) + {\mathrm{Cl}}_2 \left(\mathrm{g}\right)$ is attained at $25°\mathrm{C}$ in a closed container and inert gas helium is introduced. Which of the following statements are correct?

For the reaction ${\mathrm{PCl}}_5 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3 \left(\mathrm{g}\right) + {\mathrm{Cl}}_2 \left(\mathrm{g}\right)$, the forward reaction at constant temperature is favoured by

The equilibrium $2{\mathrm{Cu}}^{\mathrm{I}} \rightleftharpoons {\mathrm{Cu}}^0 + {\mathrm{Cu}}^{\mathrm{II}}$ in aqueous medium at $25°\mathrm{C}$ shifts towards the left in the presence of

The thermal dissociation equilibrium of ${\mathrm{CaCO}}_3 \left(\mathrm{s}\right)$ is studied under different conditions.
${\mathrm{CaCO}}_3 \left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO} \left(\mathrm{s}\right) + {\mathrm{CO}}_2 \left(\mathrm{g}\right)$ 
For this equilibrium, the correct statement (s) is (are)

For the following question, enter the correct numerical value, (in decimal-notation, truncated/rounded-off to the second decimal place, e.g., $6.25, 7.00, -0.33, 30.27, -127.30$).

The approach of the following equilibrium was observed kinetically from both directions :
${{\mathrm{PtCl}}_4}^{2-}+ {\mathrm{H}}_2\mathrm{O} \rightleftharpoons \mathrm{Pt}\left({\mathrm{H}}_2\mathrm{O}\right){{\mathrm{Cl}}_3}^{-}+{\mathrm{Cl}}^{-}$
At $25°\mathrm{C}$, it was found that $\frac{\mathrm{d} [{\mathrm{PtCl}}^{-}{]}_4}{\mathrm{dt}}=(3.90\times {10}^{-5} {\mathrm{s}}^{-1}) [{{\mathrm{PtCl}}_4}^{2-}]-(2·1\times {10}^{-3} \mathrm{L} {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}) \left[\mathrm{Pt}\right({\mathrm{H}}_2\mathrm{O}){{\mathrm{Cl}}_3}^{-}\left]\right[{\mathrm{Cl}}^{-}]$
What will be the value of the equilibrium constant when fourth ${\mathrm{Cl}}^{-}$ ion is complexed, i.e., for the step involving backward reaction?