Which is not correct relationship between ΔG⊖ and equilibrium constant KP
The reaction N2O4 (g) ⇌ 2NO2 (g) is carried out at 298 K and 20 bar. Five moles of each of N2O4and NO2, are taken initially. Given: ΔfG∘ (N2O4) = 100 kJ mol−1 and ΔfG∘ (NO2) = 50 kJ mol−1.Choose the appropriate option: The values of ΔG and K∘p at 298 K are:
For a general reaction aA(g) + bB(g) ⇋ cC(g)+ dD(g), what is the relationship between the equilibrium constants Kc and Kp? [assume Δn = μ = (c + d) - (a+b) ]\)