## Cu (s) + 2 H2SO4 (ℓ) → CuSO4 (aq) + 2 H2O (ℓ) + 1 SO2 (g)

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## 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.

 Cu             Mass: g H2SO4          Mass: g CuSO4          Mass: g H2O            Mass: g SO2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(CuSO4 (aq)) + 2ΔHf(H2O (ℓ)) + 1ΔHf(SO2 (g))] - [1ΔHf(Cu (s)) + 2ΔHf(H2SO4 (ℓ))]
[1(-844.5) + 2(-285.83) + 1(-296.83)] - [1(0) + 2(-814)] = -84.9899999999998 kJ
-84.99 kJ     (exothermic)

## Entropy Change

[1ΔSf(CuSO4 (aq)) + 2ΔSf(H2O (ℓ)) + 1ΔSf(SO2 (g))] - [1ΔSf(Cu (s)) + 2ΔSf(H2SO4 (ℓ))]
[1(-79.5) + 2(69.91) + 1(248.11)] - [1(33.15) + 2(156.9)] = -38.52 J/K
-38.52 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(CuSO4 (aq)) + 2ΔGf(H2O (ℓ)) + 1ΔGf(SO2 (g))] - [1ΔGf(Cu (s)) + 2ΔGf(H2SO4 (ℓ))]
[1(-679.11) + 2(-237.18) + 1(-300.19)] - [1(0) + 2(-690.07)] = -73.52 kJ
-73.52 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-73.51 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

7.6008722967e+012
This process is favorable at 25°C.