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Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) →...

Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K

Solutions

Expert Solution

ΔHo = -158 KJ/mol

ΔSo = -219.9 J/mol.K

= -0.2199 KJ/mol.K

T = 655 K

use:

ΔGo = ΔHo - T*ΔSo

ΔGo = -158.0 - 655.0 * -0.2199

ΔGo = -13.9655 KJ/mol

T = 655 K

ΔGo = -13.9655 KJ/mol

ΔGo = -13965.5 J/mol

use:

ΔGo = -R*T*ln Kc

-13965.5 = - 8.314*655.0* ln(Kc)

ln Kc = 2.5645

Kc = 13

Answer: 13

queen_honey_blossom answered 2 years ago
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