# Problem: Estimate the value of the equilibrium constant at 620 K for each of the following reactions. ΔG°f for BrCl(g) is ≅ 1.0 kJ/mol.(1) 2 NO2(g) ⇌ N2O4(g). ΔH°f for N2O4(g) is 9.16 kJ/mol.(2) Br2(g) + Cl2(g) ⇌ 2 BrCl(g) .ΔH°f for BrCl(g) is 14.6 kJ/mol.Express your answer using three significant figures.

###### FREE Expert Solution

We’re being asked to determine the equilibrium constant (K) at 620 K for the given reaction:

Br2(g) + Cl2(g)  2 BrCl(g)

Recall that ΔG˚rxn and K are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

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###### Problem Details

Estimate the value of the equilibrium constant at 620 K for each of the following reactions. Δf for BrCl(g) is ≅ 1.0 kJ/mol.

(1) 2 NO2(g) ⇌ N2O4(g). ΔH°f for N2O4(g) is 9.16 kJ/mol.

(2) Br2(g) + Cl2(g) ⇌ 2 BrCl(g)H°f for BrCl(g) is 14.6 kJ/mol.

Express your answer using three significant figures.