InterviewSolution
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InterviewSolution
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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? |
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Answer» 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)` |
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