TS EAMCET · Chemistry · Chemical Equilibrium

For a reaction $2 A_{(g)} ⇌ 2 B_{(g)} + C_{(g)}, K_{c} = 3.75 \times 10^{- 6}$ at $1069 K$ . The approximate value of $K_{p}$ for this reaction at the same temperature is $(R = 0.082 L bar {mol}^{- 1} K^{- 1})$

A $2.4 \times 10^{- 4}$
B $3.3 \times 10^{- 4}$
C $33 \times 10^{2}$
D $7.2 \times 10^{34}$

Verified Solution

Answer & Solution

Correct Answer

(B) $3.3 \times 10^{- 4}$

Step-by-step Solution

Detailed explanation

Equilibrium constant in terms of concentration (Kc) and in terms of partial pressure (Kp) are related as, Kp=Kc(RT)∆n Δn= number of gaseous moles of product - number of gaseous moles of reactant ∆n=3-2=1 Hence, Kp=3.75×10-6×0.082×1069…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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For a reaction 2A(g)⇌2B(g)+C(g),Kc=3.75×10-6 at 1069 K. The approximate value of Kp for this reaction at the same temperature is R=0.082 Lbarmol-1 K-1

Step-by-step Solution

For a reaction $2 A_{(g)} ⇌ 2 B_{(g)} + C_{(g)}, K_{c} = 3.75 \times 10^{- 6}$ at $1069 K$ . The approximate value of $K_{p}$ for this reaction at the same temperature is $(R = 0.082 L bar {mol}^{- 1} K^{- 1})$