What is the equilibrium constant `K_(c)` for the following reaction at `400K`?
`2NOCI(g) hArr 2NO(g) +CI_(2)(g)`
`DeltaH^(Theta) = 77.2 kJ mol^(-1)` and `DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K`.

What is the equilibrium constant K_(eq) for the following reaction at 400 K. 2NOCl_((g)) hArr 2NO_((g)) +Cl_(2(g)) , given that DeltaH^0=77.2 "kJ mol"^(-1) and DeltaS^0=122 "JK"^(-1) "mol"^(-1) .

Write the expression for the equilibrium constant K_c for the following reactions. 2NOCI(g) harr 2NO(g) + Cl_2(g)

What is the value of the equilibrium constant for the following reaction at 400 K ? 2NOCl(g) hArr 2NO(g) + Cl_(2)(g) Delta H^(@) = 77.5 kJ mol^(-1), R = 8.3124 J mol^(-1) K^(-1), Delta S = 135 J K^(-1) mol^(-1) .

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .