Consider a reaction: A(g)+B(g)⇌C(g)+D(g)
A(g),B(g) and
C(g) are taken in a container at 1 bar partial pressure each and adequate amount of liquid 'D' is added.
From the data given below. Calculate a+b+c+d
Given :
ΔG0fA(g)=30 kJ\ mole−1; ΔG0fB(g)= 20 kJ mole−1;
ΔG0fC(g)= 50 kJ mole−1; ΔG0fD(g)= 100 kJ mole−1;
Vapour pressure of D(l) at 300 K=16 bar [All data at 300 K]
where
a = Equilibrium constant of the given reaction
b = Twice the partial pressure of A at equilibrium
c = Twice the partial pressure of B at equilibrium
d = Twice the partial pressure of C at equilibrium