Question

At `500^(@)C` the equilibrium constant for the reaction
`N_(2)(g) + 3H_(2) (g) hArr 2NH_(3)(g) is 6.02 xx 10^(-2) litre^(-2) mol^(-2)`
What is the value of `K_(p)` at the same temperature?

Answer 1

According to the available data :
`K_(c) = 6.02 xx 10^(-2) litre^(-2) mol^(-2), Delta ng = 2-4 = -2.`
`R=0.082 " litre atm " K^(-1) mol^(-1), T=500^(@)C = 773 K `
By using the relation ` K_(p) = K_(c) (RT) Delta ng `
`= (6.02 xx 10^(-2) litre^(-2) mol^(-2)) xx (0.082 " litre atm " K^(-1) mol^(-1) xx 773 K)^(-2)`
` = 1.5 xx 10^(-5) atm^(-2)`