Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(g). A2(g) + B2(g) leftharpoons 2 AB(g) At equilibrium, the concentration of A2 = 3.0 × 10-3 M of B2 = 4.2 × 10-3 M of AB = 2.8 × 10-3 M If the reaction takes place in a sealed vessel at 527° C, then the value of KC will be :

Question

Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(g). A2(g) + B2(g) leftharpoons 2 AB(g) At equilibrium, the concentration of A2 = 3.0 × 10-3 M of B2 = 4.2 × 10-3 M of AB = 2.8 × 10-3 M If the reaction takes place in a sealed vessel at 527° C, then the value of KC will be : (A) 1.9 (B) 0.62 (C) 4.5 (D) 2.0

Tardigrade Admin · Accepted Answer

A2 + B2 leftharpoons 2AB Kc = ([AB]2/[A2][B2]) = (2.8 × 2.8 × 10-6/3 × 10-3 × 4.2 × 10-3) = 0.62

1.9

0.62

4.5

2.0

A2​+B2​⇌2AB Kc​=[A2​][B2​][AB]2​=3×10−3×4.2×10−32.8×2.8×10−6​=0.62

$A_{2} + B_{2} ⇌ 2 A B$
$K_{c} = \frac{[ A B ] ^{2}}{[ A _{2} ] [ B _{2} ]} = \frac{2.8 \times 2.8 \times 1 0 ^{- 6}}{3 \times 1 0 ^{- 3} \times 4.2 \times 1 0 ^{- 3}} = 0.62$