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At 500^(@)C the equilibrium constant for...

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?

Text Solution

AI Generated Solution

To find the value of \( K_p \) for the reaction \[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \] given that the equilibrium constant \( K_c \) at \( 500^\circ C \) is \( 6.02 \times 10^{-2} \, \text{litre}^{-2} \, \text{mol}^{-2} \), we can use the relationship between \( K_p \) and \( K_c \): ...
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