Chemical EquilibriumHard
Question
For the equilibrium at 298 K; N2O4(g) ⇋ 2NO2(g); G-N2O4 = 100 kJ mol-1 and G-NO2 = 50 kJ mol-1. If 5 mol of N2O4 and 2 moles of NO2 are taken initially in one liter container than which statement are correct.
Options
A.Reaction proceeds in forward direction
B.Kc = 1
C.ᐃG = - 0.55 KJ, ᐃG- = 0
D.At equilibrium [N2O4] = 4.84 M and [NO2] = 0.212 M
Solution
ᐃG = ᐃG- + 2.303 RT log Q
ᐃG = 2 × G-NO2 - G-N2O4 = 2 × 50 - 100 = 0
∴ ᐃG = 0 + 2.303 × 8.314 × 10-3 × 298 log
= 0 - 0.55 kJ
∴ ᐃG = -0.55 kJ, i.e., reaction proceed in forward direction
Also ᐃG- = 0 = 2.303 RT log K ∴ K = 1
Now, N2O4 - 2NO2
5 2
5 - x 2 + 2x
∴ Kp =
or x = 0.106
ᐃG = 2 × G-NO2 - G-N2O4 = 2 × 50 - 100 = 0
∴ ᐃG = 0 + 2.303 × 8.314 × 10-3 × 298 log
= 0 - 0.55 kJ
∴ ᐃG = -0.55 kJ, i.e., reaction proceed in forward direction
Also ᐃG- = 0 = 2.303 RT log K ∴ K = 1
Now, N2O4 - 2NO2
5 2
5 - x 2 + 2x
∴ Kp =
or x = 0.106Create a free account to view solution
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