## Sn (s white) + 2 HCl (aq) → SnCl2 (aq) + H2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Sn             Mass: g HCl            Mass: g or Solution Volume: mL of Concentration: mol/L SnCl2          Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(SnCl2 (aq)) + 1ΔHf(H2 (g))] - [1ΔHf(Sn (s white)) + 2ΔHf(HCl (aq))]
[1(-343.1) + 1(0)] - [1(0) + 2(-167.15)] = -8.80000000000001 kJ
-8.80 kJ     (exothermic)

## Entropy Change

[1ΔSf(SnCl2 (aq)) + 1ΔSf(H2 (g))] - [1ΔSf(Sn (s white)) + 2ΔSf(HCl (aq))]
[1(95.96) + 1(130.59)] - [1(51.55) + 2(56.48)] = 62.04 J/K
62.04 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(SnCl2 (aq)) + 1ΔGf(H2 (g))] - [1ΔGf(Sn (s white)) + 2ΔGf(HCl (aq))]
[1(-289.7) + 1(0)] - [1(0) + 2(-131.25)] = -27.2 kJ
-27.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-27.30 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

58277.241426
This process is favorable at 25°C.

## Reference(s):

Halka, Monica and Nordstrom, Brian. Metals & Metalloids; Infobase Publishing: New York, NY, 2011; pg. 49.