Assertion :For the reaction $A (g) ⇌ B (g) + C (g)$ , $K_{p} = 1 a t m$ . If we start with equal moles of all gases at 9 atm of initial pressure, then at equilibrium partial pressure of A increases. Reason: Reaction quotient $Q_{p} > K_{p}$ hence equilibrium shifts in a backward direction.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
For the reaction $A (g) ⇌ B (g) + C (g)$ , $K_{p} = 1 a t m$ . If we start with equal moles of all gases at 9 atm of initial pressure, then at equilibrium partial pressure of A increases.
Reaction quotient $Q_{p} > K_{p}$ hence equilibrium shifts in a backward direction.
Since, the number of moles of A, B and C are equal, their mole fractions will be 0.33 each and their partial pressures will be $0.33 \times 9 = 3 a t m$ each.

The reaction quotient will be $Q_{P} = \frac{P_{B} P_{C}}{P_{A}} = \frac{3 \times 3}{3} = 3 a t m .$ It is greater than $K_{P}$ of 1 atm. The product concentration is much higher than the reactant concentration.

Hence, the equilibrium will shift in the backward direction so that more products will be converted to reactants. This will continue till product concentration becomes equal to the equilibrium concentration.
Thus, both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Assertion :For the reaction A(g)⇌B(g)+C(g),Kp=1atm. If we start with equal moles of all gases at 9 atm of initial pressure, then at equilibrium partial pressure of A increases. Reason: Reaction quotient Qp>Kp hence equilibrium shifts in a backward direction.

Assertion :For the reaction $A (g) ⇌ B (g) + C (g)$ , $K_{p} = 1 a t m$ . If we start with equal moles of all gases at 9 atm of initial pressure, then at equilibrium partial pressure of A increases. Reason: Reaction quotient $Q_{p} > K_{p}$ hence equilibrium shifts in a backward direction.