## MgBr2 (aq) + 2 AgNO3 (aq) → 2 AgBr (s) + Mg(NO3)2 (aq)

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## Reaction Type:

Double Displacement

## 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.

 MgBr2          Mass: g or Solution Volume: mL of Concentration: mol/L AgNO3          Mass: g or Solution Volume: mL of Concentration: mol/L AgBr           Mass: g Mg(NO3)2       Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(AgBr (s)) + 1ΔHf(Mg(NO3)2 (aq))] - [1ΔHf(MgBr2 (aq)) + 2ΔHf(AgNO3 (aq))]
[2(-100.37) + 1(-881.57)] - [1(-709.95) + 2(-101.78)] = -168.8 kJ
-168.80 kJ     (exothermic)

## Entropy Change

[2ΔSf(AgBr (s)) + 1ΔSf(Mg(NO3)2 (aq))] - [1ΔSf(MgBr2 (aq)) + 2ΔSf(AgNO3 (aq))]
[2(107.11) + 1(154.81)] - [1(26.77) + 2(219.12)] = -95.98 J/K
-95.98 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(AgBr (s)) + 1ΔGf(Mg(NO3)2 (aq))] - [1ΔGf(MgBr2 (aq)) + 2ΔGf(AgNO3 (aq))]
[2(-96.9) + 1(-677.48)] - [1(-662.74) + 2(-34.22)] = -140.1 kJ
-140.10 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-140.18 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.5141785356e+024
This process is favorable at 25°C.