Chapter 7

In the reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})\), when \(100 \mathrm{~mL}\) of \(\mathrm{N}_{2}\) has reacted, the volumes of \(\mathrm{H}_{2}\) and \(\mathrm{NH}_{3}\) are (a) \(300 \mathrm{~mL}\) of \(\mathrm{H}_{2}\) and \(300 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) (b) \(100 \mathrm{~mL}\) of \(\mathrm{H}_{2}\) and \(200 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) (c) \(300 \mathrm{~mL}\) of \(\mathrm{H}_{2}\) and \(200 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) (d) \(100 \mathrm{~mL}\) of \(\mathrm{H}\), and \(100 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\)

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

For the reaction, \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\), the rate con- stants 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 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) \(8.33\)

In the reaction \(2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{S}_{2}(\mathrm{~g})\) the concentration of \(\mathrm{H}_{2} \mathrm{~S}\) is \(0.5 \mathrm{~mol} \mathrm{~L}^{-1}\) and concentration of \(\mathrm{H}_{2}\) is \(0.1 \mathrm{~mol} \mathrm{~L}^{-1}\) while concentration of \(\mathrm{S}_{2}\) is \(0.4\) \(\operatorname{mol} \mathrm{L}^{-1}\) in one litre vessel. The value of equilibrium constant of the reaction is (a) \(0.016\) (b) \(0.013\) (c) \(0.020\) (d) \(0.030\)

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 \(\mathrm{K}_{2}\) then (a) \(\mathrm{K}_{1}=\mathrm{K}_{2}\) (b) \(\mathrm{K}_{1}=2 \mathrm{~K}_{2}\) (c) \(\mathrm{K}_{2}=\sqrt{\mathrm{K}_{1}}\) (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 \(1.2 \mathrm{~atm}\). The value of \(\mathrm{K}_{\mathrm{p}}\) for this reaction is (a) \(2.4 \mathrm{~atm}\) (b) \(6.2 \mathrm{~atm}^{-2}\) (c) \(4.2 \mathrm{~atm}^{-1}\) (d) \(8.4 \mathrm{~atm}^{-3}\)

In which of the following gaseous reaction, \(\mathrm{K}_{\mathrm{p}}\) and \(\mathrm{K}_{\mathrm{c}}\) have the same values? (a) \(2 \mathrm{Hl} \rightleftharpoons \mathrm{H}_{2}+\mathrm{I}_{2}\) (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) \(\mathrm{PCI}_{5} \rightleftharpoons \mathrm{PCI}_{3}+\mathrm{Cl}_{2}\)

In which of the following gaseous reaction, the value of \(K_{p}\) is less than \(K_{c}\) ? (a) \(\mathrm{PCl}_{3} \rightleftharpoons \mathrm{PCI}_{3}+\mathrm{Cl}_{2}\) (b) \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}\) (c) \(2 \mathrm{HI} \rightleftharpoons{ } \mathrm{H}_{2}+\mathrm{I}_{2}\) (d) \(\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}\)

The value of \(K_{p}\) for the reaction, \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}\) at 700 is \(1.3 \times 10^{-3} \mathrm{~atm}^{-1} .\) The value of \(K_{c}\) at same temperature will be (a) \(1.4 \times 10^{-2}\) (b) \(7.4 \times 10^{-2}\) (c) \(5.2 \times 10^{-2}\) (d) \(3.1 \times 10^{-2}\)

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) RT (d) 1

If \(2 \mathrm{NO} \rightleftharpoons \mathrm{N}_{2}+\mathrm{O}_{2}\) \(\mathrm{K}_{c_{1}}=2.5 \times 10^{\mathrm{s}}\) \(\mathrm{NO}+\frac{1}{2} \mathrm{Br}_{\mathrm{g}} \rightleftharpoons \mathrm{NOBr}\) \(\mathrm{K}_{\mathrm{c}_{2}}=1.6\) 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) \(2.02 \times 10^{15}\)

The reaction \(\mathrm{PCl}_{5}(\mathrm{~s}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})\) is in equilibrium. If the equilibrium concentration of \(\mathrm{PCI}_{3}\) (g) is doubled, then concentration of \(\mathrm{Cl}_{2}(\mathrm{~g})\) would become (a) \(1 / 2\) of its initial value (b) \(1 / 4\) of its initial value (c) four times of its initial value (d) two times of initial value

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 \(\left.\operatorname{mol} \mathrm{L}^{-1}\right)\) ? (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 \(162 \mathrm{~L}\) \(\mathrm{mol}^{-1} \mathrm{sec}^{-1}\), what is the velocity constant (in \(\mathrm{L} \mathrm{mol}^{-1}\) \(\mathrm{sec}^{-1}\) ) 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 \(0.02 \mathrm{~mol}\) \(\mathrm{L}^{-1} \min ^{-1}\). What is the rate (in \(\mathrm{mol} \mathrm{L}^{-1}, \mathrm{~min}^{-1}\) ) of the backward reaction at equilibrium? (a) \(0.04\) (b) \(0.01\) (c) \(0.02\) (d) 1

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

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) \(\mathrm{L} \rightleftharpoons \mathrm{J} ;=0.025\)

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) \(\mathrm{R}=\mathrm{P} ; \mathrm{K}=0.01\)

At Kp for the following reaction is 1 atm \(\mathrm{X}(\mathrm{g}) \rightleftharpoons \mathrm{Y}(\mathrm{g})+\mathrm{Z}(\mathrm{g})\) At equilibrium, \(50 \%\) of \(X(g)\) is dissociated. The total pressure of the equilibrium system is 'P' atm. what is the partial pressure (in atm) of \(X(\mathrm{~g})\) at equilibrium? (a) 1 (b) 4 (c) 2 (d) \(0.5\)

At \(550 \mathrm{~K}\), the \(\mathrm{K}_{c}\) for the following reaction is \(10^{4} \mathrm{~mol}^{-1}\) lit \(\mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons \mathrm{Z}(\mathrm{g})\) At equilibrium, it was observed that \([\mathrm{X}]=1 / 2[\mathrm{Y}]=1 / 2[\mathrm{Z}]\) What is the value of \([\mathrm{Z}]\left(\mathrm{in} \mathrm{mol} \mathrm{L}^{-1}\right)\) 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 \(\mathrm{K}_{c}\), 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 \(\mathrm{N}_{2} \mathrm{O}_{4}\) is dissociation to \(33 \%\) and \(40 \%\) at total pressure \(\mathrm{P}_{1}\) and \(\mathrm{P}_{2}\) atm respectively. The ratio of \(\frac{\mathrm{P}_{1}}{\mathrm{P}_{2}}\) is (a) \(\frac{8}{5}\) (b) \(\frac{5}{8}\) (c) \(\frac{9}{5}\) (d) \(\frac{5}{9}\)

If the equilibrium constant for the reaction, \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})\) at 750 is 49 , then the equilibrium constant for the reaction, \(\mathrm{NH}_{3}(\mathrm{~g}) \rightleftharpoons\) \(1 / 2 \mathrm{~N}_{2}(\mathrm{~g})+3 / 2 \mathrm{H}_{2}(\mathrm{~g})\) 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, \(\mathrm{K}_{\mathrm{P}}=\mathrm{K}_{\mathrm{c}}\) ? (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) \(\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}) ; \Delta \mathrm{H}=+\mathrm{ve}\) (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) \(\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}=+\mathrm{ve}\)

In an equilibrium reaction, \(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})\), the partial pres- sure \(\mathrm{SO}_{2}, \mathrm{O}_{2}\) and \(\mathrm{SO}_{3}\) are \(0.662,0.101\) and \(0.331 \mathrm{~atm}\) respectively. What should be the partial pressure of oxygen if the equilibrium concentration of \(\mathrm{SO}_{3}\) and \(\mathrm{SO}_{2}\) becomes equal? (a) \(0.4 \mathrm{~atm}^{-1}\) (b) \(0.6 \mathrm{~atm}^{-1}\) (c) \(0.12 \mathrm{~atm}^{-1}\) (d) \(0.8 \mathrm{~atm}^{-1}\)

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) \(-142.16 \mathrm{~kJ} / \mathrm{mole}\) (b) \(-71.08 \mathrm{~kJ} / \mathrm{mole}\) (c) \(-35.54 \mathrm{~kJ} /\) mole (d) none of these

What will be the value of equilibrium constant \(\left(\mathrm{K}_{1}\right)\) for the reaction, \(\mathrm{HI}(\mathrm{g}) \rightleftharpoons 1 / 2 \mathrm{H}_{2}(\mathrm{~g})+1 / 21_{2}(\mathrm{~g})\), if its value for the reaction \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}\) 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 \(\mathrm{H}_{2} \mathrm{PO}_{4} \longrightarrow \mathrm{H}^{+}+\mathrm{HPO}_{4}^{2-}\) 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 (K) for \(\mathrm{H}_{3} \mathrm{PO}_{4} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{PO}_{4}^{3-}\) 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) \(K_{1},+K_{2}+K_{3}\)

In a \(0.5\) litre capacity vessel, \(\mathrm{CO}\) and \(\mathrm{Cl}_{2}\) are mixed to form \(\mathrm{COCl}_{2}\). At equilibrium, it contains \(0.2 \mathrm{~mole}\) of \(\mathrm{COCl}_{2}\) and \(0.1\) mole each of \(\mathrm{CO}\) and \(\mathrm{Cl}_{2}\). The equilibrium constant \(\left(\mathrm{K}_{0}\right)\) 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 \(K_{c}\) in \(m o l L^{-1}\) 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 \(K_{c}\) 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 \(\left(\mathrm{K}_{\alpha}\right)\) 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 dissociation constants \(\left(\mathrm{K}_{d}\right)\) of two complexes (A) and (B) are given below (a) \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] ; \mathrm{K}_{\mathrm{d}}=2.6 \times 10^{37}\) (b) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] ; \mathrm{K}_{\mathrm{d}}=1.9 \times 10^{17}\) (a) \(\mathrm{A}\) and \(\mathrm{B}\) are equally stable. (b) \(\mathrm{A}\) is more stable than \(\mathrm{B}\). (c) \(\mathrm{B}\) is more stable than \(\mathrm{A}\). (d) The data is insufficient.

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 \(\mathrm{K}_{\mathrm{p}}\) 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 \(\mathrm{O}_{2}\). As soon as \(\mathrm{NO}\) and \(\mathrm{O}_{2}\) are formed they react to form \(\mathrm{N}_{2} \mathrm{O}_{5}\). Two equilibria $$ \begin{aligned} \mathrm{N}_{2} \mathrm{O}_{4} & \rightleftharpoons 2 \mathrm{NO}+\mathrm{O}_{2} \\ 2 \mathrm{NO}+\frac{3}{2} \mathrm{O}_{2} &=\mathrm{N}_{2} \mathrm{O}_{3} \end{aligned} $$ 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) \([\mathrm{NO}]+\left[\mathrm{O}_{2}\right]=\left[\mathrm{N}_{2} \mathrm{O}_{4}\right]+\left[\mathrm{N}_{2} \mathrm{O}_{3}\right]\) (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 \(\mathrm{K}_{\mathrm{P}}\) 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 \(\mathrm{l}\) atm pressure. The value of \(K\) is (a) \(0.444\) (b) \(0.555\) (c) \(0.333\) (d) \(0.666\)

\(\mathrm{K}_{\mathrm{c}}\) for the reaction \(\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})\) \+ NO (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) \(0.4,1.6\)

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

Determine the value of equilibrium constant \(\left(\mathrm{K}_{\mathrm{C}}\right.\) ) for the reaction $$ \mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g}) $$ If 10 moles of \(A_{2} ; 15\) moles of \(B_{2}\) and 5 moles of \(A B\) are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of \(\mathrm{AB}\) is \(7.5 \mathrm{M}\) : (a) \(4.5\) (b) \(1.5\) (c) \(0.6\) (d) None of these