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

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Reaction Type:

Double Displacement

Stoichiometry

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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  or Solution Volume: mL of Concentration: mol/L

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)

3.51417853559044E+24
This process is favorable at 25°C.