For the reaction, $2 A (g) + B_{2} (g) \underset{}{⇌} 2 AB (g); ΔH = - 65 .34 kJ {mol}^{- 1} {and K}_{c} = 3 .6 \times 10^{23} L {mol}^{- 1}$
Which of the following statement (s) is/are INCORRECT?
I. The value of equilibrium constant increases as the temperature increases.
II. The addition of $He (g)$ at constant pressure shifts the reaction in the backward direction.
III. The equilibrium shifts in the forward direction if pressure is increased.
IV. The large value of $K_{c}$ indicates that the reaction is almost going for completion and hence does not require any catalyst.

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II & III

III & IV

I & IV

I, II, III & IV

answer is C.

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Detailed Solution

I) Incorrect. As the reaction is exothermic, increase in temperature decreases Kc.
II) Correct. Addition of an inert gas at constant pressure drives the reaction in the direction of increasing number of moles.
III) Correct. Increase in pressure moves the reaction in the direction of decreasing number of moles.
IV) Incorrect. Value of Kc does not provide any information on rate of the reaction and hence regarding catalyst.

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