## F2 (g) + 2 KCl (aq) → 2 KF (aq) + Cl2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 F2             Mass: g or Gas Volume: L KCl            Mass: g or Solution Volume: mL of Concentration: mol/L KF             Mass: g Cl2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(KF (aq)) + 1ΔHf(Cl2 (g))] - [1ΔHf(F2 (g)) + 2ΔHf(KCl (aq))]
[2(-508.04) + 1(0)] - [1(0) + 2(-419.55)] = -176.98 kJ
-176.98 kJ     (exothermic)

## Entropy Change

[2ΔSf(KF (aq)) + 1ΔSf(Cl2 (g))] - [1ΔSf(F2 (g)) + 2ΔSf(KCl (aq))]
[2(247.98) + 1(222.97)] - [1(202.71) + 2(158.98)] = 198.26 J/K
198.26 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(KF (aq)) + 1ΔGf(Cl2 (g))] - [1ΔGf(F2 (g)) + 2ΔGf(KCl (aq))]
[2(-545.64) + 1(0)] - [1(0) + 2(-414.55)] = -262.18 kJ
-262.18 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-236.09 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

8.6001210719e+045
This process is favorable at 25°C.