For the reaction : N 2 O 4 (g) 
2NO 2 (g)
(i) In a mixture of 5 mol NO 2 and 5 mol N 2 O 4 and pressure of 20 bar. Calculate the value of Δ G for the reaction. Given Δ G f ° (NO 2 ) = 50 kJ / mol, Δ G f ° (N 2 O 4 ) = 100 kJ / mol and T = 298 K.
(ii) Predict the direction in which the reaction will shift, in order to attain equilibrium
[Given at T = 298 K, 2.303 RT = 5.7 kJ / mol.]
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
(i) Δ G = 5.7 kJ/mol (ii) backward shifting
Sol. (i) Δ Gº for the reaction
Δ Gºreac. = 2 Δ Gº ƒ (NO 2 ) – Δ Gº ƒ (N 2 O 4 )
100 – 100 = 0
Now, Δ G = 2.303 RT log Q P + Δ Gº
Here Q P = 
= 
= 10 atm
So, Δ G = 2.303 RT log Q P + 0 = 2.303 RT log Q P = 2.303 RT log 10 10= 2.303 RT = 5.7 kJ/mole
(ii) Since Q P is more than K P
(calculate K P by putting the value of Δ Gº in the equation Δ Gº = 2.303 RT log K P as Δ Gº = 0 that’s why K P comes as 1.)
Hence, the reaction will proceed in backward direction.
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