For the system A(g) +2B(g) leftharpoons C(g), the equilibrium concentrations are A = 0.06 mol L-1, B = 0.12 mol L-1, C = 0.216 mol L-1 The Keq for the reaction is

Question

For the system A(g) +2B(g) leftharpoons C(g), the equilibrium concentrations are A = 0.06 mol L-1, B = 0.12 mol L-1, C = 0.216 mol L-1 The Keq for the reaction is (A) 250 (B) 416 (C) 4 × 10-3 (D) 125

Tardigrade Admin · Accepted Answer

K-([C]/[A][B]2)=(0.216/0.06×(0.12)2)=250

Q. For the system $A_{(g)} + 2 B_{(g)} ⇌ C_{(g)}$ , the equilibrium concentrations are
$A = 0.06 m o l L^{- 1}, B = 0.12 m o l L^{- 1}, C = 0.216 m o l L^{- 1}$ The $K_{e q}$ for the reaction is

$250$

$416$

$4 \times 1 0^{- 3}$

$125$

$K - \frac{[ C ]}{[ A ] [ B ] ^{2}} = \frac{0.216}{0.06 \times ( 0.12 ) ^{2}} = 250$

Q. For the system A(g)​+2B(g)​⇌C(g)​, the equilibrium concentrations are A=0.06molL−1,B=0.12molL−1,C=0.216molL−1 The Keq​ for the reaction is

250

416

4×10−3

125