Estimate the value of the equilibrium constant at 655 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K.
PART A: 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol.
PART B: Br2(g)+Cl2(g)⇌2BrCl(g) .ΔH∘f for BrCl(g) is 14.6 kJ/mol.
Part-A
2NO2(g) --------------- N2O4(g)
ΔH∘ rxn = ΔH0f of N2O4 - 2 x ΔH∘ f of NO2
ΔH∘ rxn = 9.16 - 2 x33.18
ΔH∘rxn = - 57.2KJ
ΔS0 rxn = ΔS0f of N2O4 - 2 xΔS0f of NO2
ΔS0rxn = 304.18 - 2x 239.95
ΔS0 rxn = - 175.72J
ΔG0rxn = ΔH0rxn - T ΔS0 rxn
ΔG0rxn = - 57.2 KJ - 298x(-175.72)
ΔG0rxn = - 4835.44 K
ΔG0rxn = - 4.835 KJ
ΔG0rxn = - RTlnK R= 8.314x10^-3KJ T= 655K
- 4.835 = - 8.314x10^-3 x 655x lnK
lnK = 0.888
K = e^0.889
K = 2.43.
part-B
Br2(g) + Cl2(g) --------------- 2 BrCl(g)
ΔG0rxn = -1.0KJ
ΔG0rxn = - RTlnK
-1.0 = - 8.314x10^-3 x 655x lnK
lnK = 0.183
K = e^0.183
K= 1.20
Estimate the value of the equilibrium constant at 655 K for each of the following reactions....
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