Chapter 7

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

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

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) \(\mathrm{K}_{\mathrm{p}}=\frac{\mathrm{P}\left(\mathrm{CO}_{2}\right) \times \mathrm{P}(\mathrm{Mg} \mathrm{O})}{\mathrm{P}(\mathrm{MgCO})_{3}}\)

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

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) \(\frac{1}{i \mathrm{~K}_{c}}\)

\(\mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g}) ; \Delta \mathrm{H}=+\mathrm{ve}\), 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

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

\(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})\) 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) \(\mathrm{K}_{0}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{-2}\)

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) \(\mathrm{K}_{\mathrm{c}}=\mathrm{K}_{\mathrm{p}}(\mathrm{RT})^{3}\)

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

A reversible reaction is said to have attained equilibrium, when (a) backward reaction stops (b) both backward and forward reactions take place at equal speed (c) both backward and forward reactions stop (d) concentration of each of the reactants and products becomes equal

The equilibrium between water and its vapour, in an open vessel (a) can be achieved (b) depends upon pressure (c) cannot be achieved (d) depends upon temperature

Which of the following equilibrium, in gaseous phase, would be unaffected by an increase in pressure? (a) \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) (b) \(\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4} \rightleftharpoons 2 \mathrm{NO}_{2}\) (d) \(\mathrm{CO}_{2}+{ }^{1} / 2 \mathrm{O}_{2} \rightleftharpoons \mathrm{CO}_{2}\)

Amongst the following hydroxides, the one which has the lowest value of \(K_{s p}\) at ordinary temperature (about \(25^{\circ} \mathrm{C}\) ) is (a) \(\mathrm{Mg}(\mathrm{OH})_{2}\) (b) \(\mathrm{Ca}(\mathrm{OH})_{2}\) (c) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (d) \(\mathrm{Be}(\mathrm{OH})_{2}\)

A saturated solution of non-radioactive sugar was taken and a little radioactive sugar was added to it. A small amount of it gets dissolved in solution and an equal amount of sugar was precipitated. This proves (a) the equilibrium has been established in the solution (b) radioactive sugar can displace non-radioactive sugar from its solution. (c) Equilibrium is dynamic in nature (d) none of the above

The relation between \(\mathrm{K}_{\mathrm{p}}\) and \(\mathrm{K}_{c}\) for the reaction \(2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NOCl}(\mathrm{g})\) is (a) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{-1}\) (b) \(\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}\) (c) \(K_{P}-K_{e} /(R T)^{2}\) (d) \(K_{p}=K_{c} / R T\)

When two reactants \(\mathrm{A}\) and are mixed to give products and \(D\), the reaction quotient \(Q\), at the initial stages of the reaction (a) is zero (b) decreases with time (c) is independent of time (d) increases with time

When a catalyst is added to a reversible reaction in equilibrium state, the value of equilibrium constant (a) increases (b) decreases (c) does not change (d) becomes zero

A vessel at equilibrium, contains \(\mathrm{SO}_{3}, \mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\), Now some helium gas is added, so that total pressure increases while temperature and volume remain constant. According to Le Chatelier's Principle, the dissociation of \(\mathrm{SO}_{3}\) (a) decreases (b) remains unaltered (c) increases (d) change unpredictably

In a reversible reaction, the catalyst (a) decreases activation energy of forward reaction (b) increases activation energy of forward reaction (c) decreases activation energy of both forward and backward reactions (d) increases activation energy of backward reaction

A chemical reaction is catalysed by a catalyst \(\mathrm{X}\). Hence, \(\mathrm{X}\) (a) increases activation energy of the reaction (b) does not affect equilibrium constant of the reaction (c) decreases rate constant of the reaction (d) reduces enthalpy of the reaction

If for the reaction given below \(2 \mathrm{PQ} \rightleftharpoons{\mathrm{B}} \rightleftharpoons{\mathrm{P}_{2}}+\underset{\mathrm{g}}{\mathrm{Q}_{2}} \mathrm{~K}_{1}=2.5 \times 10^{5}\) \(\mathrm{PQ}+\frac{1}{2} \mathrm{R}_{2} \rightleftharpoons{\mathrm{PQR}} \mathrm{K}_{2}=5 \times 10^{-3}\) find \(\mathrm{K}_{3}\) for the reaction \(\frac{1}{2} \mathrm{P}_{2}+\frac{1}{2} \mathrm{Q}_{2}+\frac{1}{2} \mathrm{R}_{2} \rightleftharpoons \mathrm{PQR}\) (a) \(2.5 \times 10^{-3}\) (b) \(2.5 \times 10^{3}\) (c) \(1 \times 10^{-3}\) (d) \(5 \times 10^{-3}\)

For equilibrium reaction \(2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})+14.6 \mathrm{~J}\), increase in tem- perature would (a) favour the formation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) (b) stop reaction (c) favour the decomposition of \(\mathrm{N}_{2} \mathrm{O}_{4}\) (d) no alter the equilibrium

Which of the following favours the backward reaction in a chemical equilibrium? (a) decreasing the concentration of one of the reactants (b) increasing the concentration of one of the reactants (c) increasing the concentration of one or more of the products (d) removal of at least one of the products at regular intervals

If an inert gas is added in the reaction \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) at constant volume, then its equilibrium (a) remains unaffected (b) favours the backward reaction (c) favours the forward reaction (d) increases the dissociation of reactants

In the reaction \(\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}\) at equili- brium, some \(I_{2}\) is added. What happens to the equilibrium? (a) it gets shifted to the right (b) it remains unchanged (c) it gets shifted to the left (d) first (b) then (c)

The role of a catalyst in a reversible reaction is to (a) alter the equilibrium constant of the reaction (b) increase the rate of forward reaction (c) allow the equilibrium to be achieved quickly (d) decrease the rate of backward reaction

find \(\Delta \mathrm{G}^{\circ}\) for the reaction given below? \(\frac{1}{2} \mathrm{~A}+\frac{3}{2} \mathrm{~B} \rightleftharpoons \mathrm{C}\) \(\mathrm{K}_{\mathrm{eq}}=826 \mathrm{~atm}^{-1}\) at \(298 \mathrm{~K}\) (a) \(-8.32 \mathrm{KJ}\) (b) \(8.32 \mathrm{KJ}\) (c) \(16.64 \mathrm{KJ}\) (d) -16.64 KJ

\(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g})=\frac{\mathrm{Fe} / \mathrm{Mo}, 500^{\circ} \mathrm{C}}{=\mathrm{V} 200-900 \mathrm{~atm}} 2 \mathrm{NH}_{3}+22.4\) kcal formation of \(\mathrm{NH}_{3}\) by above reaction shows (a) Cyanamide process (b) Serpeck's process (c) Haber process (d) None of these

Which of the following reaction will be favoured at low pressure? (a) \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) (b) \(\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}\) (c) \(\mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{3}+\mathrm{Cl}_{2}\) (d) \(\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}\)

For the chemical reaction \(3 \mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons \mathrm{X}_{3} \mathrm{Y}(\mathrm{g})\), the amount of \(\mathrm{X}_{3} \mathrm{Y}\) at equilibrium is affected by (a) temperature and pressure (b) temperature only (c) pressure only (d) temperature, pressure and catalyst

At constant temperature, the equilibrium constant \(\left(\mathrm{K}_{\mathrm{p}}\right)\) for the decomposition reaction, \(\mathrm{N}_{2} \mathrm{O}_{4} \longrightarrow 2 \mathrm{NO}_{2}\) is expressed by \(\mathrm{K}_{p}=\left(4 \mathrm{x}^{2} \mathrm{P}\right) /\left(1-\mathrm{x}^{2}\right)\), where \(\mathrm{P}=\) pressure, \(\mathrm{x}=\) extent of decomposition. Which one of the following statements is true? (a) \(\mathrm{K}_{\mathrm{p}}\) increases with increase of \(\mathrm{P}\) (b) \(\mathrm{K}_{p}\) increases with increase of \(\mathrm{x}\) (c) \(K_{p}\) increases with decrease of \(x\) (d) \(\mathrm{K}_{\mathrm{p}}\) remains constant with change in \(\mathrm{P}\) and \(\mathrm{x}\)

For the reaction \(\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})\) the forward reaction at constant temperature is favoured by 1\. introducing an inert gas at constant volume 2\. introducing chlorine gas at constant volume 3\. introducing an inert gas at constant pressure 4\. increasing the volume of the container 5\. introducing \(\mathrm{PCl}_{5}\) at constant volume (a) \(1,2,3\) (b) 4,5 (c) \(2,3,5\) (d) \(3,4,5\)

For the reaction \(\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g})\) at a given temperature, the equilibrium amount of \(\mathrm{CO}_{2}(\mathrm{~g})\) can be increased by (a) adding a suitable catalyst (b) adding an inert gas (c) decreasing the volume of the container (d) increasing the amount of \(\mathrm{CO}(\mathrm{g})\)

In a reaction \(\mathrm{A}_{2}(\mathrm{~g})+4 \mathrm{~B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_{4}(\mathrm{~g}) ; \Delta \mathrm{H}<0\) The formation of \(\mathrm{AB}_{4}(\mathrm{~g})\) will be favoured by (a) low temperature and high pressure (b) high temperature and high pressure (c) low temperature and low pressure (d) high temperature and low pressure

In which of the following cases does the reaction go farthest to completion? (a) \(\mathrm{K}=1\) (b) \(\mathrm{K}=10\) (c) \(\mathrm{K}=10^{-2}\) (d) \(\mathrm{K}=10^{2}\)

Consider the following reactions: 1\. \(\mathrm{AB}_{2}(\mathrm{~g})+1 / 2 \mathrm{~B}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{AB}_{3}(\mathrm{~g})\) 2\. \(2 \mathrm{AB}_{3}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}_{2}+\mathrm{B}_{2}(\mathrm{~g})\) If and \(\mathrm{K}_{2}\) are the equilibrium constants at \(27^{\circ} \mathrm{C}\) of reactions 1 and 2 respectively, then \(\mathrm{K}\), and \(\mathrm{K}_{2}\) are related as (a) \(\mathrm{K}_{1}^{2}=\mathrm{K}_{2}\) (b) \(\mathrm{K}_{2} \mathrm{~K}_{1}^{2}=1\) (c) \(\mathrm{K}_{1}=2 \mathrm{~K}_{2}\) (d) \(K, K_{2}^{2}=1\)

Reaction quotient for the reaction, \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons-2 \mathrm{NH}_{3}(\mathrm{~g})\) is given by \(\mathrm{Q}=\frac{\left[\mathrm{NH}_{3}\right]^{2}}{\left[\mathrm{~N}_{2}\right]\left[\mathrm{H}_{2}\right]^{3}}\) the reaction will proceed from right to left, if \(\mathrm{K}_{\mathrm{c}}\) is equilibrium constant (a) \(\mathrm{Q}<\mathrm{K}_{c}\) (b) \(\mathrm{Q}=0\) (c) \(\mathrm{Q}>\mathrm{K}_{c}\) (d) \(Q=K_{c}\)

For the reaction, \(\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}\), the equilibrium concentrations of \(\mathrm{H}_{2}, 1_{2}\) and \(\mathrm{HI}\) are 8,3 and \(28 \mathrm{~mol} \mathrm{~L}^{-1}\) respectively. Equilibrium constant of the reaction is (a) \(32.67\) (b) \(31.67\) (c) \(34.67\) (d) \(36.67\)

In which of the following case, the value of \(K_{p}\) is less than \(\mathrm{K}_{\mathrm{c}}\) ? (a) \(\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}\) (b) \(\mathrm{H}_{2}+\mathrm{Cl}_{2} \rightleftharpoons 2 \mathrm{HCl}\) (c) \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}\) (d) \(\mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{3}+\mathrm{Cl}_{2}\)

For the reaction $$ \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) $$ \(\Delta_{r} \mathrm{H}=-170.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\) Which of the following statements is not true? (a) addition of \(\mathrm{CH}_{4}(\mathrm{~g})\) or \(\mathrm{O}_{2}(\mathrm{~g})\) at equilibrium will cause a shift to the right (b) the reaction is exothermic (c) at equilibrium, the concentrations of \(\mathrm{CO}_{2}(\mathrm{~g})\) and \(\mathrm{H}_{2} \mathrm{O}\) (1) are not equal (d) the equilibrium constant for the reaction is given by \(\mathrm{K}_{\mathrm{p}}=\frac{\left[\mathrm{CO}_{2}\right]}{\left[\mathrm{CH}_{4}\right]\left[\mathrm{O}_{2}\right]}\)

The enthalpy and entropy change for the reaction, \(\mathrm{Br}_{2}(1)+\mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{BrCl}(\mathrm{g})\) are \(30 \mathrm{~kJ} \mathrm{~mol}^{-1}\) and \(105 \mathrm{~J} \mathrm{~mol}^{-1}\) respectively. The temperature at which the reaction will be in equilibrium is (a) 450 (b) 300 (c) \(285.7\) (d) 273

If \(K_{1}\) and \(K_{2}\) are the respective equilibrium constants for the two reactions, \(\mathrm{XeF}_{6}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})=\mathrm{XeOF}_{4}(\mathrm{~g})+2 \mathrm{HF}(\mathrm{g})\) \(\mathrm{XeO}_{4}(\mathrm{~g})+\mathrm{XeF}_{6}(\mathrm{~g}) \rightleftharpoons \mathrm{XeOF}_{4}(\mathrm{~g})+\mathrm{XeO}_{3} \mathrm{~F}_{2}(\mathrm{~g})\) Then equilibrium constant of the reaction \(\mathrm{XeO}_{4}(\mathrm{~g})+\) \(2 \mathrm{HF}(\mathrm{g}) \rightleftharpoons \mathrm{XeO}_{3} \mathrm{~F}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) will be (a) \(\mathrm{K}_{1} /\left(\mathrm{K}_{2}\right)^{2}\) (b) \(\mathrm{K}_{1} \cdot \mathrm{K}_{2}\) (c) \(\mathrm{K}_{1} / \mathrm{K}_{2}\) (d) \(\mathrm{K}_{2} / \mathrm{K}_{\mathrm{t}}\)

For the reaction, \(\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}\) the equilibrium concentration of \(\mathrm{H}_{2}, \mathrm{I}_{2}\) and \(\mathrm{HI}\) are \(8.0,3.0\) and \(28.0\) mole/litre, respectively, the equilibrium constant is (a) \(28.34\) (b) \(32.66\) (c) \(34.78\) (d) \(38.88\)

In a chemical equilibrium rate constant of forward reaction is \(7.5 \times 10^{-4}\) and the equilibrium constant is 1.5. The rate constant of backward reaction is (a) \(2.5 \times 10^{4}\) (b) \(5 \times 10^{-4}\) (c) \(2.5 \times 10^{-4}\) (d) \(5 \times 10^{4}\)

The equilibrium constant for the reaction, \(\mathrm{SO}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g})\) is \(K_{c}=4.9 \times 10^{-2} .\) The value of \(K_{c}\) for the reaction \(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})\) will be (a) 416 (b) \(2.40 \times 10^{-3}\) (c) \(9.8 \times 10^{-2}\) (d) \(4.9 \times 10^{-2}\)

The value of \(K_{p}\) for the reaction, \(2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{S}_{2}(\mathrm{~g})\) is \(1.2 \times 10^{-2}\) at \(1065{ }^{\circ} \mathrm{C}\). The value for \(\mathrm{K}_{\mathrm{c}}\) is (a) \(<1.2 \times 10^{-2}\) (b) \(>1.2 \times 10^{-2}\) (c) \(1.2 \times 10^{-2}\) (d) \(0.12 \times 10^{-2}\)

The equilibrium constant for the following reaction will be \(3 \mathrm{~A}+2 \mathrm{~B}=\mathrm{C}\) (a) \(\frac{[3 \mathrm{~A}][2 \mathrm{~B}]}{[\mathrm{C}]}\) (b) \(\frac{[\mathrm{C}]}{[3 \mathrm{~A}][2 \mathrm{~B}]}\) (c) \(\frac{[\mathrm{C}]}{[\mathrm{A}]^{2}[\mathrm{~B}]^{2}}\) (d) \(\frac{[\mathrm{C}]}{[\mathrm{A}]^{3}[\mathrm{~B}]^{2}}\)

The equilibrium constant of a reaction is 300 . If the volume of reaction flask is tripled, the equilibrium constant is (a) 300 (b) 600 (c) 900 (d) 100

One mole of HI was heated in a sealed tube at \(440^{\circ} \mathrm{C}\) till the equilibrium was reached. HI was found to be \(22 \%\) decomposed. The equilibrium constant for dissociation reaction, \(2 \mathrm{HI} \rightleftharpoons \mathrm{H}_{2}+\mathrm{I}_{2}\) is (a) \(1.99\) (b) \(0.282\) (c) \(0.01988\) (d) \(0.0796\)