2 Li (s) + 2 H2O (ℓ) → 2 LiOH (aq) + 2 H2 (g)

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Reaction Type:

Single displacement/Oxidation-reduction

Stoichiometry

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Li             Mass: g
H2O            Mass: g
LiOH           Mass: g
H2             Mass: g  or Gas Volume: L
Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(LiOH (aq)) + 2ΔHf(H2 (g))] - [2ΔHf(Li (s)) + 2ΔHf(H2O (ℓ))]
[2(-508.49) + 2(0)] - [2(0) + 2(-285.83)] = -445.32 kJ
-445.32 kJ     (exothermic)

Entropy Change

[2ΔSf(LiOH (aq)) + 2ΔSf(H2 (g))] - [2ΔSf(Li (s)) + 2ΔSf(H2O (ℓ))]
[2(2.65) + 2(130.59)] - [2(29.1) + 2(69.91)] = 68.46 J/K
68.46 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(LiOH (aq)) + 2ΔGf(H2 (g))] - [2ΔGf(Li (s)) + 2ΔGf(H2O (ℓ))]
[2(-450.58) + 2(0)] - [2(0) + 2(-237.18)] = -426.8 kJ
-426.80 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-465.73 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

5.9742798375e+074
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 299.

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