We’re being asked to determine the **equilibrium constant (K)** at **298.15 K** for the given reaction:

HCl(g) + NH_{3}(g) → NH_{4}Cl(s)

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

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

We can use the following equation to solve for ** ΔG˚_{rxn}**:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

Consider the reaction

HCl (g) + NH_{3} (g) → NH_{4}Cl (s)

Using the Standard thermodynamic data, calculate the equilibrium constant for this reaction at 298.15 K.

ANSWER: ____________

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