Question

tionThe table below gives the equilibrium concentrations for this reaction at acertain temperature:N (9) +0,0).22NO(9)[N][02][NO]0.69 M0.98 M0.034 MWhat is the equilibrium constant for the reaction?A. 9.9B. 1.7 x 10-3

Answer 1

k = 1.7 x 10^-3

Explanations:

Given the the reaction between nitrogen and oxygen gas expressed as:

`N_2(g)+O_2(g)\rightarrow2NO(g)`

The equilibrium constant for the reaction is expressed as:

`k=([NO]^2)/([N_2[O_2])`

Given the following concentrations

[NO] = 0.034M

[N2] = 0.69

[O2] = 0.98

Substitute the concentrations into the formula to have:

`\begin{gathered} k=(0.034^2)/(0.69*0.98) \\ k=(0.001156)/(0.6762) \\ k=0.0017 \\ k=1.7*10^(-3) \end{gathered}`

Hence the equilibrium constant for the reaction is 1.7 x 10^-3