For a reaction 2 A(g) leftharpoons 2 B(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 L. bar mol -1 K -1 )

Question

For a reaction 2 A(g) leftharpoons 2 B(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 L. bar mol -1 K -1 ) (A) 2.4 × 10-4 (B) 3.3 × 10-4 (C) 33 × 102 (D) 7.2 × 104

Tardigrade Admin · Accepted Answer

Kp is related to KC by the formula. Kp=KC(R T)Δ n For the equation 2 A ( g ) leftharpoons 2 B(g)+C(g) Δ n=(2+1)-2=1 R =0.082 l text bar mol -1 K -1 T =1069 K KC =375 × 10-6 Substituting the values in equation and solving we get Kp=3.3 × 10-4

Q. For a reaction $2 A (g) ⇌ 2 B (g) + C (g)$
$K_{C} = 3.75 \times 1 0^{- 6}$ at $1069 K .$ The approximate value of $K_{p}$ for this reaction at the same temperature is $(R = 0.082 L$ bar $m o l^{- 1} K^{- 1}$ )

$2.4 \times 1 0^{- 4}$

$3.3 \times 1 0^{- 4}$

$33 \times 1 0^{2}$

$7.2 \times 1 0^{4}$

Q. For a reaction 2A(g)⇌2B(g)+C(g) KC​=3.75×10−6 at 1069K. The approximate value of Kp​ for this reaction at the same temperature is (R=0.082L bar mol−1K−1 )

2.4×10−4

3.3×10−4

33×102

7.2×104

Kp​ is related to KC​ by the formula. Kp​=KC​(RT)Δn For the equation 2A(g)⇌2B(g)+C(g) Δn=(2+1)−2=1 R=0.082l bar mol−1K−1 T=1069K KC​=375×10−6 Substituting the values in equation and solving we get Kp​=3.3×10−4

Q. For a reaction $2 A (g) ⇌ 2 B (g) + C (g)$
$K_{C} = 3.75 \times 1 0^{- 6}$ at $1069 K .$ The approximate value of $K_{p}$ for this reaction at the same temperature is $(R = 0.082 L$ bar $m o l^{- 1} K^{- 1}$ )

$2.4 \times 1 0^{- 4}$

$3.3 \times 1 0^{- 4}$

$33 \times 1 0^{2}$

$7.2 \times 1 0^{4}$