Problem 1
The reaction \(\mathrm{PCl}_{5}(\mathrm{~g})=\mathrm{PCl}_{3}(\mathrm{~s})+\mathrm{Cl}_{2}(\mathrm{~g})\) is an example of (a) backward reaction (b) forward reaction (c) irreversible reaction (d) reversible reaction
Problem 2
For a reversible reaction, if the concentrations of the reactants are doubled, at constant temperature the equilibrium constant will be (a) one-fourth (b) halved (c) doubled (d) the same
Problem 3
The value of \(K_{p}\) in the reaction \(\mathrm{MgCO}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{MgO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})\) is (a) \(\mathrm{K}_{\mathrm{p}}=\mathrm{P}\left(\mathrm{CO}_{2}\right)\) (b) \(\mathrm{K}_{\mathrm{p}}=\frac{\mathrm{P}\left(\mathrm{MgCO}_{3}\right)}{\mathrm{P}\left(\mathrm{CO}_{2}\right) \times \mathrm{P}(\mathrm{Mg} \mathrm{O})}\) (c) \(K_{p}=\frac{P\left(C O_{2}\right) \times P\left(C O_{2}\right) \times P(M g O)}{P(M g C O)_{3}}\) (d) \(\mathrm{K}_{\mathrm{p}}=\frac{\mathrm{P}\left(\mathrm{CO}_{2}\right) \times \mathrm{P}(\mathrm{Mg} \mathrm{O})}{\mathrm{P}(\mathrm{MgCO})_{3}}\)
Problem 4
In the reaction \(\mathrm{BaO}_{2}(\mathrm{~s}) \rightleftharpoons \mathrm{BaO}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g})\) \(\Delta \mathrm{H}=\) tve. In equilibrium condition, pressure of \(\mathrm{O}_{2}\) depends on (a) increase mass of \(\mathrm{BaO}_{2}\) (b) increase mass of \(\mathrm{BaO}\) (c) temperature of equilibrium (d) mass of \(\mathrm{BaO}_{2}\) and \(\mathrm{BaO}\) both
Problem 6
If equilibrium constant for the reaction \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) is \(\mathrm{K}_{\mathrm{c}}\), then the equilibrium con- stant for the reaction \(\mathrm{NH}_{3}=1 / 2 \mathrm{~N}_{2}+\frac{3}{2} \mathrm{H}_{2}\) will be (a) \(\frac{1}{\mathrm{~K}_{\mathrm{c}}}\) (b) \(\frac{1}{\mathrm{~K}^{2}}\) (c) \(\sqrt{K}\) (d) \(\frac{1}{i \mathrm{~K}_{c}}\)
Problem 7
\(\mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g}) ; \Delta \mathrm{H}=+\mathrm{ve}\), it (a) increase by pressure (b) it occurs at \(1000 \mathrm{~atm}\) pressure (c) it occurs at high temperature (d) it occurs at high pressure and temperature
Problem 8
For a reversible reaction, the concentration of the reactants are doubled, then the equilibrium constant (a) becomes one-fourth (b) is doubled (c) is halved (d) remains same
Problem 9
\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})\) in the above reaction \(\mathrm{K}_{\mathrm{p}}\) and \(\mathrm{K}_{\mathrm{c}}\) are related as (a) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})\) (b) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{-1}\) (c) \(\mathrm{K}_{\mathrm{c}}=\mathrm{K}_{\mathrm{p}} \times(\mathrm{RT})^{2}\) (d) \(\mathrm{K}_{0}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{-2}\)
Problem 10
In the reaction, \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+\) heat, relation- ship between \(K_{p}\) and \(K_{c}\) is (a) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-2}\) (b) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{c}(\mathrm{RT})^{2}\) (c) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-3}\) (d) \(\mathrm{K}_{\mathrm{c}}=\mathrm{K}_{\mathrm{p}}(\mathrm{RT})^{3}\)
Problem 11
Which of the following change will shift the reaction in forward direction? \(\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons-21(\mathrm{~g})\) Take \(\Delta \mathrm{H}^{\circ}=+150 \mathrm{~kJ}\) (a) increase in concentration of \(I\) (b) increase in total pressure (c) decrease in concentration of \(\mathrm{I}_{2}\) (d) increase in temperature
