For the given equilibrium reaction, 2 Ag⇌2 Bg+Cg the equilibrium constant K_c at 1000 K is 4×10^(-4). Calculate K_p for the reaction at 800 K temperature

Q13 / 160 · TS EAMCET 2020 (09 Sep Shift 1) · Chemistry

For the given equilibrium reaction,
$2 A (g) ⇌ 2 B (g) + C (g)$
the equilibrium constant $(K_{c})$ at $1000 K$ is $4 \times 10^{- 4}$ . Calculate $K_{p}$ for the reaction at $800 K$ temperature

Relation between Kp and Kc

$K_{p} = K_{c} {(R T)}^{∆ n}$ .

$R = 0.082$ $T = 800 K$ $∆ n = 1$ $K_{c} = 4 \times 10^{- 4}$

$K_{p} = 0.0004 \times (0.082 \times 800) = 0.026$

Hence, the correct answer is option: 'B'.