Chapter 7

If a mixture containing 3 moles of hydrogen and 1 mole of nitrogen is converted completely into ammonia, the ratio of volumes of reactants and products at the same temperature and pressure would be (a) \(2: 1\) (b) \(1: 2\) (c) \(1: 3\) (d) \(3: 1\)

The ratio of \(\mathrm{K}_{p} / \mathrm{K}_{c}\) for the reaction \(\mathrm{CO}(\mathrm{g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})\) is (a) (b) RT (c) \((\mathrm{RT})^{L / 2}\) (d) \((\mathrm{RT})^{-1 / 2}\)

For the reaction, \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\), the rate constants for the forward and backward reactions are found to be \(4.2 \times 10^{-2}\) and \(3.36 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) respectively. What is the equilibrium constant for the reaction? (a) \(11.5\) (b) \(12.5\) (c) \(8.0\) (d) \(6.0\)

The vapour density of \(\mathrm{N}_{2} \mathrm{O}_{4}\) at a certain temperature is 30\. What is the percentage dissociation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) at this temperature? (a) \(53.3\) (b) \(106.6\) (c) \(26.7\) (d) none of these

The rate constants for the forward and backward reactions of hydrolysis of ester are \(1.1 \times 10^{-2}\) and \(1.5 \times 10^{-3}\) mol \(\mathrm{L}^{-1} \mathrm{~s}^{-1}\) respectively. The equilibrium constant of the reaction, \(\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+\mathrm{H}^{+} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+\) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) is (a) \(6.53\) (b) \(7.34\) (c) \(7.75\) (d) \(8.33\)

If equilibrium constants of reaction, \(\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}\) is \(\mathrm{K}_{1}\), and \(1 / 2 \mathrm{~N}_{2}+1 / 2 \mathrm{O}_{2} \rightleftharpoons \mathrm{NO}\) is \(K_{2}\) then (a) \(\mathrm{K}_{1}=\mathrm{K}_{2}\) (b) \(\mathrm{K}_{1}=2 \mathrm{~K}_{2}\) (c) \(\mathrm{K}_{2}=\sqrt{\mathrm{K}}\) (d) \(\mathrm{K}_{1}=1 / 2 \mathrm{~K}_{2}\)

For a gaseous reaction \(2 \mathrm{~A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\), the partial pressures of \(\mathrm{A}, \mathrm{B}, \mathrm{C}\) and \(\mathrm{D}\) at equilibrium are \(0.5\), \(0.8,0.7\) and \(1.2\) atm. The value of \(K_{p}\) for this reaction is (a) \(2.4 \mathrm{~atm}\) (b) \(6.2 \mathrm{~atm}^{-2}\) (c) \(4.2 \mathrm{~atm}^{-1}\) (d) \(8.4 \mathrm{~atm}^{-3}\)

For the reaction \(\mathrm{C}_{(s s}+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})\), the par- tial pressures of \(\mathrm{CO}\), and \(\mathrm{CO}\) are 4 and 8 atm respectively. The value of \(K_{ }^{\prime}\) for this reaction is (a) \(14 \mathrm{~atm}\) (b) \(16 \mathrm{~atm}\) (c) \(18 \mathrm{~atm}\) (d) \(12 \mathrm{~atm}\)

In which of the following gaseous reaction, \(\mathrm{K}_{0}\) and \(\mathrm{K}_{\mathrm{c}}\) have the same values? (a) \(2 \mathrm{H} 1 \rightleftharpoons \mathrm{H}_{2}+\mathrm{I}_{2}\) (b) \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\) (c) \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}\) (d) \(\mathrm{PCI}_{5}=\mathrm{PCI}_{3}+\mathrm{Cl}_{2}^{3}\)

The ratio of \(\mathrm{Kp} / \mathrm{Kc}\) for the reaction \(\mathrm{SO}_{2}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})\) is (a) \((\mathrm{RT})^{-1 / 2}\) (b) \((\mathrm{RT})^{1 / 2}\) (c) \(\mathrm{RT}\) (d)

If \(2 \mathrm{NO} \rightleftharpoons \mathrm{N}_{2}+\mathrm{O}_{2}\) \(\mathrm{K}_{c_{1}}=2.5 \times 10^{30}\) \(\mathrm{NO}+\frac{1}{2} \mathrm{Br}_{2} \rightleftharpoons \mathrm{NOBr}\) \(\mathrm{K}_{c_{2}}=1.6\) find \(K_{c}\) for the reaction given below \(\frac{1}{2} \mathrm{~N}_{2}+\frac{1}{2} \mathrm{O}_{2}+\frac{1}{2} \mathrm{Br}_{2} \rightleftharpoons \mathrm{NOBr}\) (a) \(1.01 \times 10^{-15}\) (b) \(2.02 \times 10^{-15}\) (c) \(1.01 \times 10^{30}\) (d) \(2.02 \times 10^{15}\)

\(9.2\) grams of \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})\) is taken in a closed one litre vessel and heated till the following equilibrium is reached \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g}) .\) At equilibrium, \(50 \%\) of \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})\) is dissociated. What is the equilibrium constant (in \(\mathrm{mol} \mathrm{L}^{-1}\) )? (molecular weight of \(\mathrm{N}_{2} \mathrm{O}_{4}\) is 92 ) (a) \(0.1\) (b) \(0.2\) (c) \(0.4\) (d) 2

Equilibrium constant for the reaction \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})\) is 81. If the velocity constant of the forward reaction is \(162 \mathrm{~L}\) \(\mathrm{mol}^{-1} \sec ^{-1}\), what is the velocity constant (in \(\mathrm{L} \mathrm{mol}^{-1}\) \(\sec ^{-1}\) ) for the backward reaction? (a) 13122 (b) 2 (c) 261 (d) 243

One mole of \(\mathrm{A}(\mathrm{g})\) is heated to \(300^{\circ} \mathrm{C}\) in a closed one litre vessel till the following equilibrium is reached. \(\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})\) The equilibrium constant of this reaction at \(300^{\circ} \mathrm{C}\) is 4 . What is the concentration of \(\mathrm{B}\) (in \(\mathrm{mol} \mathrm{L}^{-1}\) ) at equilibrium? (a) \(0.2\) (b) \(0.6\) (c) \(0.75\) (d) \(0.1\)

One mole of \(\mathrm{A}(\mathrm{g})\) is heated to \(200{ }^{\circ} \mathrm{C}\) in a one litre closed flask, till the following equilibrium is reached. \(\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})\) The rate of forward reaction at equilibrium is \(0.02 \mathrm{~mol}\) \(\mathrm{L}^{-1} \mathrm{~min}^{-1}\). What is the rate (in mol \(\mathrm{L}^{-1}, \mathrm{~min}^{-1}\) ) of the backward reaction at equilibrium? (a) \(0.04\) (b) \(0.01\) (c) \(0.02\) (d) 1

In the reaction \(\mathrm{PCl}_{5}(\mathrm{~g})=\mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})\), the equilibrium concentrations of \(\mathrm{PC} 1_{5}\) and \(\mathrm{PCl}_{3}\) are \(0.4\) and \(0.2\) mole/litre respectively. If the value of \(K\) is \(0.5\), what is the concentration of \(\mathrm{Cl}_{2}\) in mole/ litre? (a) \(2.0\) (b) \(1.5\) (c) \(1.0\) (d) \(0.5\)

Consider the following reaction equilibrium \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})\) Initially, 1 mole of \(\mathrm{N}_{2}\) and 3 mole of \(\mathrm{H}_{2}\) are taken in a 2 litre flask. At equilibrium state, if the number of union of \(\mathrm{N}_{2}\) in \(0.6\), what is the total number of moles of all gases present in the flask? (a) \(0.8\) (b) \(1.6\) (c) \(3.2\) (d) \(6.4\)

In which of the following reactions, the concentration of reactant is equal to concentration of product at equilibrium \((\mathrm{K}=\) equilibrium constant \() ?\) (a) \(\mathrm{A} \rightleftharpoons \mathrm{B} ; \mathrm{K}=0.01\) (b) \(\mathrm{R} \rightleftharpoons \mathrm{P} ; \mathrm{K}=1\) (c) \(\mathrm{X} \rightleftharpoons \mathrm{Y} ; \mathrm{K}=10\) (d) \(L \rightleftharpoons \quad J ;=0.025\)

In which of the following reactions, the concentration of product is higher than the concentration of reactant at equilibrium? = equilibrium constant) (a) \(\mathrm{A} \rightleftharpoons \mathrm{B} ; \mathrm{K}=0.001\) (b) \(\mathrm{M} \rightleftharpoons \mathrm{N} ; \mathrm{K}=10\) (c) \(\mathrm{X} \rightleftharpoons \mathrm{Y} ; \mathrm{K}=0.005\) (d) \(\mathrm{R} \longrightarrow \mathrm{P} ; \mathrm{K}=0.01\)

At \(550 \mathrm{~K}\), the \(\mathrm{K}\) for the following reaction is \(10^{4} \mathrm{~mol}^{-1}\) lit \(\mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons{\rightleftharpoons}{\rightleftharpoons} \mathrm{Z}(\mathrm{g})\) At equilibrium, it was observed that \([\mathrm{X}]=1 / 2[\mathrm{Y}]=1 / 2[\mathrm{Z}]\) What is the value of \([\mathrm{Z}]\) (in \(\mathrm{mol} \mathrm{L}^{-1}\) ) at equilibrium? (a) \(2 \times 10^{-4}\) (b) \(10^{-4}\) (c) \(2 \times 10^{4}\) (d) \(10^{4}\)

4 moles each of \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) gases are allowed to react to form \(\mathrm{SO}_{3}\) in a closed vessel. At equilibrium \(25 \%\) of \(\mathrm{O}_{2}\) is used up. The total number of moles of all the gases at equilibrium is (a) \(6.5\) (b) \(7.0\) (c) \(8.0\) (d) \(2.0\)

For the reversible reaction, \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons=2 \mathrm{NH}_{3}(\mathrm{~g})\) At \(500{ }^{\circ} \mathrm{C}\), the value of \(\mathrm{K}_{\mathrm{p}}\) is \(1.44 \times 10^{-5}\) when partial pressure is measured in atmospheres. The corresponding value of \(\mathrm{K}_{i}\), with concentration in mole \(\mathrm{L}^{-1}\), is (a) \(1.44 \times 10^{-5} /(0.082 \times 500)^{-2}\) (b) \(1.44 \times 10^{-5} /(8.314 \times 773)^{-2}\) (c) \(1.44 \times 10^{-5}(0.082 \times 773)^{2}\) (d) \(1.44 \times 10^{-5} /(0.082 \times 773)^{-2}\)

If the equilibrium constant for the reaction, \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g})=2 \mathrm{NH}_{3}(\mathrm{~g})\) at 750 is 49 , then the equilibrium constant for the reaction, \(\mathrm{NH}_{3}(\mathrm{~g})=\) \(1 / 2 \mathrm{~N}_{2}(\mathrm{~g})+3 / 2 \mathrm{H}_{2}(\mathrm{~g})\) at the same temperature will be (a) \(1 / 49\) (b) 49 (c) \(1 / 7\) (d) \(49^{2}\)

For the reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}), \Delta \mathrm{H}=-93.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\) the concentration of \(\mathrm{H}_{2}\) at equilibrium can be increased by (i) lowering the temperature (ii) increasing the volume of the system (iii) adding \(\mathrm{N}_{2}\) at constant volume (iv) adding \(\mathrm{H}_{2}\) at constant volume (a) (ii) and (iv) are correct (b) only (ii) is correct (c) (i), (ii) and (iii) are correct (d) (iii) and (iv) are correct

For which of the following reaction, \(K_{p}=K_{c} ?\) (a) \(2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})\) (b) \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})\) (c) \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HCl}(\mathrm{g})\) (d) \(\mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{5}(\mathrm{~g})\)

In which of the following reactions, equilibrium is independent of pressure? (a) \(\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})=2 \mathrm{NO}(\mathrm{g}) ; \Delta \mathrm{H}=+\mathrm{ve}\) (b) \(2 \mathrm{SO}_{2}+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}\) (c) \(3 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{N}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}=-\mathrm{ve}\) (d) \(\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons{\rightleftharpoons} \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}=+\mathrm{ve}\)

The equilibrium constant of mutarotation of \(\alpha\)-D-glucose to \(\beta\)-D-glucose is \(1.8 .\) What per cent of the \(\alpha\)-form remains under equilibrium? (a) \(35.7\) (b) \(64.3\) (c) \(55.6\) (d) \(44.4\)

The equilibrium constant for the reaction \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{S}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})\) is \(18.5\) at 925 and \(9.25\) at 1000 respectively. What is the enthalpy of the reaction? (a) \(-142.16 \mathrm{~kJ} /\) mole (b) \(-71.08 \mathrm{~kJ} /\) mole (c) \(-35.54 \mathrm{~kJ} / \mathrm{mole}\) (d) none of these

For a gaseous equilibrium \(2 \mathrm{~A}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{(\mathrm{g})}, \mathrm{K}_{\mathrm{p}}\) has a value of \(1.8 \mathrm{at}\) \(700 \mathrm{~K}\). What is the value of \(\mathrm{K}_{c}\) for the equilibrium \(2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{~A}\) at the same pressure? (a) \(0.031\) (b) \(1.3 \times 10^{-3}\) (c) \(44.4\) (d) 38

What will be the value of equilibrium constant \(\left(\mathrm{K}_{1}\right)\) for the reaction, \(\mathrm{HI}(\mathrm{g})=1 / 2 \mathrm{H}_{2}(\mathrm{~g})+1 / 2 \mathrm{I}_{2}(\mathrm{~g})\), if its value for the reaction \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons{ }_{2} \mathrm{2HI}\) is \(64 ?\) (a) \(1 / 64\) (b) \(1 / 8\) (c) 64 (d) 8

The equilibrium constant for the reaction \(\mathrm{H}_{3} \mathrm{PO}_{4} \rightleftharpoons \mathrm{H}^{+}+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)is \(\mathrm{K}_{1}\), for reaction \(\mathrm{H}_{2} \mathrm{PO}_{4} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HPO}_{4}^{2-}\) is \(\mathrm{K}_{2}\) and for reaction \(\mathrm{HPO}_{4}^{2-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{PO}_{4}^{3-}\) is \(\mathrm{K}_{3} .\) The equilibrium constant \((\mathrm{K})\) for \(\mathrm{H}_{3} \mathrm{PO}_{4} \rightleftharpoons 3 \mathrm{H}^{+}+\mathrm{PO}_{4}^{3-}\) will be (a) \(\mathrm{K}_{1}, \times \mathrm{K}_{2} \times \mathrm{K}_{3}\) (b) \(\mathrm{K}_{1} / \mathrm{K}_{2} \mathrm{~K}_{3}\) (c) \(\mathrm{K}_{2} / \mathrm{K}_{1} \mathrm{~K}_{3}\) (d) \(K_{1},+K_{2}^{1}+K_{3}\)

The equilibrium constants for the reactions, \(\mathrm{XeF}_{6}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons{\mathrm{XeOF}}_{4}(\mathrm{~g})+2 \mathrm{HF}(\mathrm{g})\) (i) and \(\mathrm{XeO}_{4}(\mathrm{~s})+\mathrm{XeF}_{6}(\mathrm{~g}) \rightleftharpoons{=} \mathrm{XeOF}_{4}(\mathrm{~g})+\) \(\mathrm{XeO}_{3} \mathrm{~F}_{2}(\mathrm{~g}) \ldots .\) (ii) are \(\mathrm{K}_{1}\) and \(\mathrm{K}_{2}\) respectively. The equilibrium constant \((\mathrm{K})\) for the reaction \(\mathrm{XeO}_{4}(\mathrm{~g})+2 \mathrm{HF}(\mathrm{g}) \rightleftharpoons \mathrm{XeO}_{3} \mathrm{~F}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) is (a) \(\mathrm{K}_{1} / \mathrm{K}\) (b) \(\mathrm{K}_{2} / \mathrm{K}_{1}\) (c) \(\mathrm{K}_{1} / \mathrm{K}_{2}\) (d) \(\mathrm{K}_{1} / \mathrm{K}_{2}\)

HI was heated in sealed tube at \(400^{\circ} \mathrm{C}\) till the equilibrium was reached. HI was found to be \(22 \%\) decomposed. The equilibrium constant for dissociation is (a) \(1.99\) (b) \(0.0199\) (c) \(0.0796\) (d) \(0.282\)

In a \(0.5\) litre capacity vessel, \(\mathrm{CO}\) and \(\mathrm{Cl}\), are mixed to form \(\mathrm{COCl}_{2} .\) At equilibrium, it contains \(0.2\) mole of \(\mathrm{COCl}_{2}\) and \(0.1\) mole each of \(\mathrm{CO}\) and \(\mathrm{Cl}_{2}\). The equilibrium constant \(\left(\mathrm{K}_{c}\right)\) for reaction \(\mathrm{CO}+\mathrm{Cl}_{2} \rightleftharpoons \mathrm{COCl}_{2}\) is (a) 15 (b) 5 (c) 20 (d) 10

One mole of \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})\) at 300 is kept in a closed container under one atmosphere. It is heated to 600 when \(20 \%\) by mass of \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})\) decomposes to \(\mathrm{NO}_{2}\) (g). The resultant pressure is (a) \(1.2 \mathrm{~atm}\) (b) \(2.4 \mathrm{~atm}\) (c) \(2.0 \mathrm{~atm}\) (d) \(1.0 \mathrm{~atm}\)

An equilibrium mixture for the reaction, \(2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{S}_{2}(\mathrm{~g})\) had 1 mole of \(\mathrm{H}_{2} \mathrm{~S}, 0.2\) mole of \(\mathrm{H}_{2}\) and \(0.8\) mole of \(\mathrm{S}_{2}\) in a 2 litre flask. The value of \(\mathrm{K}_{\varepsilon}\) in \(\mathrm{mol} \mathrm{L}^{-1}\) is (a) \(0.08\) (b) \(0.016\) (c) \(0.004\) (d) \(0.160\)

\(1.25\) moles of NOCl were placed in a \(2.50 \mathrm{~L}\) reaction chamberat \(427^{\circ} \mathrm{C}\). After equilibrium was reached, \(1.10\) moles of \(\mathrm{NOCl}\) remained. Calculate the equilibrium constant \(K\) for the reaction, \(2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})\) (a) \(1.6 \times 10^{-3}\) (b) \(5.6 \times 10^{-4}\) (c) \(2.6 \times 10^{-3}\) (d) \(4.6 \times 10^{-4}\)

What is the correct sequence of active masses in increasing order in gaseous mixture, containing one gram per litre of each of the following? 1\. \(\mathrm{NH}_{3}\) 2\. \(\mathrm{N}_{2}\) 3\. \(\mathrm{H}_{2}\) 4\. \(\mathrm{O}_{2}\) Select the correct answer using the codes given below: (a) \(3,1,4,2\) (b) \(3,4,2,1\) (c) \(2,1,4,3\) (d) \(4,2,1,3\)

If equilibrium constant for the reaction, \(\mathrm{XO}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1) \rightleftharpoons \mathrm{HXO}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})\) is \(0.36 \times 10^{-6}\) then find the value of dissociation constant \(\left(\mathrm{K}_{a}\right)\) for \(\mathrm{HXO} ?\) (a) \(0.36 \times 10^{-8}\) (b) \(2.8 \times 10^{-8}\) (c) \(2.8 \times 10^{-10}\) (d) \(0.36 \times 10^{-6}\)

The equilibrium constant value for the reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})\) is \(1.48 \times 10^{-5}\), the value for the reaction \(1 / 2 \mathrm{~N}_{2}(\mathrm{~g})+3 / 2 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})\) is \(\mathrm{n} \times 10^{-3}\) where \(\mathrm{n}\) is (a) \(1.85\) (b) \(3.85\) (c) \(4.85\) (d) 10

A gaseous phase reaction is allowed to attain equilibrium as \(\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})\) at constant pressure P. The partial pressure of A at equilibrium is \(\mathrm{P} / 2 .\) The value of equilibrium constant \(K_{p}\) is (a) \(\frac{\mathrm{P}}{8}\) (b) \(\frac{\mathrm{P}}{6}\) (c) \(\frac{\mathrm{P}}{2}\) (d) \(\frac{\mathrm{P}}{4}\)

Two moles of \(\mathrm{N}_{2} \mathrm{O}_{4}\) is heated to form \(\mathrm{NO}\) and \(\mathrm{O}_{4}\). As soon as \(\mathrm{NO}\) and \(\mathrm{O}_{2}\) are formed they react to form \(\mathrm{N}_{2} \mathrm{O}_{5}\). Two equilibria \(\mathrm{N}_{2} \mathrm{O}_{4} \rightleftharpoons 2 \mathrm{NO}+\mathrm{O}_{2}\) \(2 \mathrm{NO}+\frac{3}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{3}\) Are simultaneously established. At equilibrium, the degree of dissociation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) was found to \(50 \%\). Which of the following is correct at equilibrium? (a) \(\frac{1}{2}[\mathrm{NO}]=\frac{3}{2}\left[\mathrm{O}_{2}\right]\) (b) \(2\left[\mathrm{~N}_{2} \mathrm{O}_{4}\right]=[\mathrm{NO}]+\frac{3}{2}\left[\mathrm{O}_{2}\right]+\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) (c) \([\mathrm{NO}]+\left[\mathrm{O}_{2}\right]=\left[\mathrm{N}_{2} \mathrm{O}_{4}\right]+\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]\) (d) \(\frac{1}{2}\left[\mathrm{~N}_{2} \mathrm{O}_{5}\right]+\left[\mathrm{O}_{2}\right]=\frac{1}{2}[\mathrm{NO}]\)

\(\mathrm{NH}_{4} \mathrm{HS}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})\) The equilibrium pressure at \(25^{\circ} \mathrm{C}\) is \(0.660 \mathrm{~atm} .\) What is \(K_{p}\) for the reaction? (a) \(0.109\) (b) \(0.218\) (c) \(1.89\) (d) \(2.18\)

\(\mathrm{PCl}_{5}\) is \(50 \%\) dissociated at \(20{ }^{\circ} \mathrm{C}\) and 1 atm pressure. The value of \(\mathrm{K}_{p}\) is (a) \(0.444\) (b) \(0.555\) (c) \(0.333\) (d) \(0.666\)

\(\mathrm{K}_{c}\) for the reaction \(\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})\) \(+\mathrm{NO}(\mathrm{g})\) is 16 at a given temperature. If we take one mole each of all the four gases in one litre vessel, the equilibrium concentration of \(\mathrm{SO}_{2}\) and \(\mathrm{SO}_{3}\) respectively in \(\operatorname{mol} \mathrm{L}^{-1}\) are (a) \(0.4,0.8\) (b) \(0.8,1.6\) (c) \(1.6,0.8\) (d) \(0.4,1.6\)

A \(1 \mathrm{M}\) solution of glucose reaches dissociation equilibrium given below. $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \rightleftharpoons 6 \mathrm{HCHO} $$ If the equilibrium constant is \(0.167 \times 10^{-22}\), the concentration of HCHO in the equilibrium is (a) \(1.60 \times 10^{-8} \mathrm{M}\) (b) \(3.20 \times 10^{-6} \mathrm{M}\) (c) \(3.20 \times 10^{-4} \mathrm{M}\) (d) \(1.60 \times 10^{-4} \mathrm{M}\)

For the dissociation reaction \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})\) the degree of dissociation \((\alpha)\) in terms of \(\mathrm{K}_{\mathrm{p}}\) and total equilibrium pressure P is: (a) \(\alpha=\sqrt{\frac{4 P+K_{\text {p }}}{K_{p}}}\) (b) \(\alpha=\sqrt{\frac{\mathrm{K}_{\mathrm{p}}}{4 \mathrm{P}+\mathrm{K}_{\mathrm{p}}}}\) (c) \(\alpha=\sqrt{\frac{\mathrm{K}_{\mathrm{p}}}{4 \mathrm{P}}}\) (d) None of these

The equilibrium constant \(\mathrm{K}_{\mathrm{P}_{1}}\) and \(\mathrm{K}_{\mathrm{p}}\) for the reactions, \(\mathrm{X}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Y}(\mathrm{g})\) and \(\mathrm{Z}(\mathrm{g}) \rightleftharpoons \mathrm{P}(\mathrm{g})+\mathrm{Q}(\mathrm{g})\) respectively are in the ratio of \(1: 9\). If the degree of dissociation of \(\mathrm{X}\) and \(\mathrm{Z}\) be equal then the ratio of total pressures at these equilibria is: (a) \(1: 36\) (b) \(1: 9\) (c) \(1: 3\) (d) \(1: 1\)

At certain temperature compound \(\mathrm{AB}_{2}(\mathrm{~g})\) dissociates according to the reaction $$ 2 \mathrm{AB}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})+\mathrm{B}_{2}(\mathrm{~g}) $$ The value of \(K_{p}\) in terms of degree of dissociation ' \(\alpha\) ' and total pressure ' \(\mathrm{P}\) ' is (a) \(\mathrm{P} \frac{\alpha^{3}}{2}\) (b) \(\mathrm{P} \frac{\alpha^{2}}{3}\) (c) \(\mathrm{P} \frac{\alpha^{3}}{3}\) (d) \(\mathrm{P} \frac{\alpha^{2}}{2}\)

When \(\mathrm{NaNO}_{3}(\mathrm{~d}=2.0 \mathrm{~g} / \mathrm{cc})\) is heated in a closed vessel of \(100 \mathrm{ml}\), oxygen is liberated and \(\mathrm{NaNO}_{2}\) \((\mathrm{d}=1.5 \mathrm{~g} / \mathrm{cc})\) is left behind as per the reaction \(2 \mathrm{NaNO}_{3}(\mathrm{~s}) \rightleftharpoons 2 \mathrm{NaNO}_{2}(\mathrm{~s})+\mathrm{O}_{2}(\mathrm{~g}) .\) At equilibrium the volumes of NaNO, left and NaNO \(_{3}\) left and NaNO, produced are very small and can be neglected. Which of the following is a correct statement about this equilibrium? (a) Addition of \(30 \mathrm{~g}\) of \(\mathrm{NaNO}_{3}\) favours reverse reaction. (b) Addition of \(30 \mathrm{~g}\) of \(\mathrm{NaNO}_{2}\) favours forward reaction. (c) Increasing temperature favours reverse reaction. (d) None of these.