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?

At 773 K, the equilibrium constant K_(c) for the reaction, N_(2) (g) + 3 H_(2) (g) hArr 2 NH_(3) (g)" is " 6.02 xx 10^(-2)L^(2) mol^(-2). Calculate the value of K_(p) at the same temperature.

At 500^@C , the equilibrium constant for the the reaction. N_(2(g))+3H_(2(g))overset (Delta)underset (Catalyst)rarr 2NH_(3(g)) is 6.02 xx10^(-2) L^(-2) mol^(-2) . What is the value of K_p at the same temperature?

(K_(c))/(K_(p)) for the reaction, N_(2)(g)+3H_(2)(g)hArr2NH_(3(g)) is

At 800 K, the equilibrium constant for the reaction, N_2(g) + 3H_2(g) hArr 2NH_3(g) is 6.05xx10^(-2)L^2 "mol"^(-2) . Calculate K_p for the reaction at the same temperature.

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , the units of K_(p) are …………

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , the units of K_(p) are …………

The equilibrium constant K_(P) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 8.19xx10^(2) at 298K and 4.6xx10^(-1) at 498 K. Calculate DeltaH^(@) fror the reaction.