For the reaction, N2(g) + O2(g) leftharpoons 2NO(g), equilibrium constant K1. 2NO(g) + O2(g) leftharpoons 2NO2(g), equilibrium constant K2 What is K for the reaction, NO2(g) leftharpoons (1/2) N2(g) + O2(g)

Question

For the reaction, N2(g) + O2(g) leftharpoons 2NO(g), equilibrium constant K1. 2NO(g) + O2(g) leftharpoons 2NO2(g), equilibrium constant K2 What is K for the reaction, NO2(g) leftharpoons (1/2) N2(g) + O2(g)  (A)  (1/K1 K2)  (B)  (1/4K2 K2)  (C) [ (1/K1 K2)]1/2 (D)  (1/2K1 K2)

Tardigrade Admin · Accepted Answer

mathrmN2+ mathrmO2 leftharpoons 2 mathrmNO ; K1 2 mathrmNO+ mathrmO2 leftharpoons 2 mathrmNO2 ; K2 mathrmNO2 leftharpoons (1/2) mathrm~N2+ mathrmO2 ; K K1=([ mathrmNO]2/[ mathrm~N2][ mathrmO2]) ; K2=([ mathrmNO2]2/[ mathrmNO]2[ mathrmO2]) K=([ mathrmN2]1 / 2[ mathrmO2]/[ mathrmNO2])=√([ mathrmN2][ mathrmO2] ×[ mathrmNO]2[ mathrmO2]/[ mathrmNO]2 ×[ mathrmNO2]2) K=√(1/K1 K2)

Q. For the reaction,
$N_{2 (g)} + O_{2 (g)} ⇌ 2 N O_{(g)},$ equilibrium constant $K_{1} .$
$2 N O_{(g)} + O_{2 (g)} ⇌ 2 N O_{2 (g)}$ , equilibrium constant $K_{2}$
What is K for the reaction,
$N O_{2 (g)} ⇌ \frac{1}{2} N_{2 (g)} + O_{2 (g)}$

$\frac{1}{K _{1} K _{2}}$

$\frac{1}{4 K _{2} K _{2}}$

$[\frac{1}{K _{1} K _{2}}]^{1/2}$

$\frac{1}{2 K _{1} K _{2}}$

Q. For the reaction, N2(g)​+O2(g)​⇌2NO(g)​, equilibrium constant K1​. 2NO(g)​+O2(g)​⇌2NO2(g)​, equilibrium constant K2​ What is K for the reaction, NO2(g)​⇌21​N2(g)​+O2(g)​

K1​K2​1​

4K2​K2​1​

[K1​K2​1​]1/2

2K1​K2​1​

N2​+O2​⇌2NO;K1​ 2NO+O2​⇌2NO2​;K2​ NO2​⇌21​ N2​+O2​;K K1​=[ N2​][O2​][NO]2​;K2​=[NO]2[O2​][NO2​]2​ K=[NO2​][N2​]1/2[O2​]​=[NO]2×[NO2​]2[N2​][O2​]×[NO]2[O2​]​​ K=K1​K2​1​​

Q. For the reaction,
$N_{2 (g)} + O_{2 (g)} ⇌ 2 N O_{(g)},$ equilibrium constant $K_{1} .$
$2 N O_{(g)} + O_{2 (g)} ⇌ 2 N O_{2 (g)}$ , equilibrium constant $K_{2}$
What is K for the reaction,
$N O_{2 (g)} ⇌ \frac{1}{2} N_{2 (g)} + O_{2 (g)}$

$\frac{1}{K _{1} K _{2}}$

$\frac{1}{4 K _{2} K _{2}}$

$[\frac{1}{K _{1} K _{2}}]^{1/2}$

$\frac{1}{2 K _{1} K _{2}}$