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For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose...

For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose 0.0600 mol NO(g), 0.0150 mol O2(g), and 1.60 mol NO2(g) are added to a rigid 2.00-L flask. What is ΔG?

Solutions

Expert Solution

molarity of NO = 0.06 / 2 = 0.03 M

molarity 0f O2 = 0.015 / 2 = 0.0075 M

molarity of NO2 = 1.60 / 2 = 0.8 M

Kp = Kc (RT)^Dn

2 x 10^-2 = Kc x (0.0821 x 638)^1

Kc = 3.82 x 10^-4

ΔGo = - RT ln Kc

         = - 8.314 x 10^-3 x 638 x ln (3.82 x 10^-4)

         = 41.75 kJ/mol

2NO2(g)    <-----------------> 2NO(g) + O2(g)

0.8                                       0.03      0.0075

Qp = [NO]^2[O2] / [NO2]^2

      = 0.03^2 x 0.0075 / 0.8^2

       = 1.05 x 10^-5

ΔG = ΔGo + RT ln Qp

      = 41.75 + 8.314 x 10^-3 x 638 x ln (1.05 x 10^-5)

      = -19 kJ/mol

ΔG = -19 kJ/mol

queen_honey_blossom answered 1 year ago
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