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

**Br**_{2(g) }+ Cl_{2(g) }⇌ 2 BrCl_{(g)}

Recall that ** ΔG˚_{rxn} and K** are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

Estimate the value of the equilibrium constant at 620 K for each of the following reactions. Δ*G°*f for BrCl_{(g)} is ≅ 1.0 kJ/mol.

(1) 2 NO_{2(g)} ⇌ N_{2}O_{4(g)}. Δ*H*°_{f} for N_{2}O_{4(g)} is 9.16 kJ/mol.

(2) Br_{2(g) }+ Cl_{2(g) }⇌ 2 BrCl_{(g)} .Δ*H*°_{f} for BrCl_{(g)} is 14.6 kJ/mol.

Express your answer using three significant figures.

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