For the reaction equilibrium, N2 O4(g) leftharpoons 2NO2(g) ; the concentration of N2O4 and NO2 at equilibrium are 4.8 × 10-2 and 1.2 × 10-2 mol/L respectively. The value of Kc for the reaction is:

Question

For the reaction equilibrium, N2 O4(g) leftharpoons 2NO2(g) ; the concentration of N2O4 and NO2 at equilibrium are 4.8 × 10-2 and 1.2 × 10-2 mol/L respectively. The value of Kc for the reaction is: (A) 3 × 10-3 M (B) 3 × 103 M (C) 3.3 × 102 M (D) 3 × 10-1 M

Tardigrade Admin · Accepted Answer

Kc =([NO2]2/[N2O4])=((1.2×10-2)2/4.8×10-2)=3.0 ×10-3 M

Q. For the reaction equilibrium,
$N_{2} O_{4 (g)} ⇌ 2 N O_{2 (g)}$ ; the concentration of $N_{2} O_{4}$ and $N O_{2}$ at equilibrium are $4.8 \times 1 0^{- 2}$ and $1.2 \times 1 0^{- 2}$ mol/L respectively. The value of Kc for the reaction is:

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

$3 \times 1 0^{3} M$

$3.3 \times 1 0_{2} M$

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

$K_{c} = \frac{[ N O _{2} ] ^{2}}{[ N _{2} O _{4} ]} = \frac{( 1.2 \times 1 0 ^{- 2} ) ^{2}}{4.8 \times 1 0 ^{- 2}} = 3.0 \times 1 0^{- 3} M$

Q. For the reaction equilibrium, N2​O4(g)​⇌2NO2(g)​ ; the concentration of N2​O4​ and NO2​ at equilibrium are 4.8×10−2 and 1.2×10−2 mol/L respectively. The value of Kc for the reaction is:

3×10−3M

3×103M

3.3×102​M

3×10−1M