Question

The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g) + O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? NO2 (g) NO (g) + 1/2 O2 (g)

Answer 1

Answer: The equilibrium constant for
`NO_2(g)\rightleftharpoons NO(g)+(1)/(2)O_2(g)` equation is
`1.36* 10^(-7)`

Step-by-step explanation:

The given chemical equation follows:

`2NO(g)+O_2(g)\rightleftharpoons 2NO_2(g)`

The value of equilibrium constant for the above equation is
`K_(eq)=5.4* 10^(13)`

Calculating the equilibrium constant for the given equation:

`NO_2(g)\rightleftharpoons NO(g)+(1)/(2)O_2(g)`

The value of equilibrium constant for the above equation will be:

`K'_(eq)=\frac{1}{\sqrt{K_(eq)}}\\\\K'_(eq)=\frac{1}{\sqrt{5.4* 10^(13)}}\\\\K'_(eq)=1.36* 10^(-7)`

Hence, the equilibrium constant for
`NO_2(g)\rightleftharpoons NO(g)+(1)/(2)O_2(g)` equation is
`1.36* 10^(-7)`