## Cl2 (g) + 2 NH4Br (aq) → 2 NH4Cl (aq) + Br2 (ℓ)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

 Cl2            Mass: g or Gas Volume: L NH4Br          Mass: g or Solution Volume: mL of Concentration: mol/L NH4Cl          Mass: g Br2            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(NH4Cl (aq)) + 1ΔHf(Br2 (ℓ))] - [1ΔHf(Cl2 (g)) + 2ΔHf(NH4Br (aq))]
[2(-299.66) + 1(0)] - [1(0) + 2(-254.06)] = -91.1999999999999 kJ
-91.20 kJ     (exothermic)

## Entropy Change

[2ΔSf(NH4Cl (aq)) + 1ΔSf(Br2 (ℓ))] - [1ΔSf(Cl2 (g)) + 2ΔSf(NH4Br (aq))]
[2(169.87) + 1(152.23)] - [1(222.97) + 2(195.81)] = -122.62 J/K
-122.62 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(NH4Cl (aq)) + 1ΔGf(Br2 (ℓ))] - [1ΔGf(Cl2 (g)) + 2ΔGf(NH4Br (aq))]
[2(-210.62) + 1(0)] - [1(0) + 2(-183.34)] = -54.56 kJ
-54.56 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-54.64 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3622682883.8
This process is favorable at 25°C.