Zn (s) + 1 H2SO4 (aq) → ZnSO4 (aq) + H2 (g)

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Reaction Type:

Single displacement/Oxidation-reduction

Stoichiometry

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 Zn             Mass: g H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L ZnSO4          Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

Enthalpy of Reaction

[1ΔHf(ZnSO4 (aq)) + 1ΔHf(H2 (g))] - [1ΔHf(Zn (s)) + 1ΔHf(H2SO4 (aq))]
[1(-1063.17) + 1(0)] - [1(0) + 1(-909.27)] = -153.9 kJ
-153.90 kJ     (exothermic)

Entropy Change

[1ΔSf(ZnSO4 (aq)) + 1ΔSf(H2 (g))] - [1ΔSf(Zn (s)) + 1ΔSf(H2SO4 (aq))]
[1(-92.02) + 1(130.59)] - [1(41.63) + 1(20.08)] = -23.14 J/K
-23.14 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(ZnSO4 (aq)) + 1ΔGf(H2 (g))] - [1ΔGf(Zn (s)) + 1ΔGf(H2SO4 (aq))]
[1(-891.73) + 1(0)] - [1(0) + 1(-744.63)] = -147.1 kJ
-147.10 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-147.00 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

5.9188727344e+025
This process is favorable at 25°C.