Mn + 2H2SO4 → MnSO4 + SO2↑ + 2H2O
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- Reaction of and sulfuric acid
The reaction of and sulfuric acid yields manganese(II) sulfate, sulfur dioxide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and sulfuric acid
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and sulfuric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing | ||
| H2SO4 | Sulfuric acid | 2 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnSO4 | Manganese(II) sulfate | 1 | Oxidized | – |
| SO2 | Sulfur dioxide | 1 | Reduced | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and sulfuric acid◆
ΔrG −351.81 kJ/mol K 4.31 × 1061 pK −61.63
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −305.76 | −351.81 | 154.3 | −13.19 |
| −305.76 | −351.81 | 154.3 | −13.19 | |
per 1 mol of | −152.88 | −175.91 | 77.15 | −6.595 |
per 1 mol of | −305.76 | −351.81 | 154.3 | −13.19 |
per 1 mol of | −305.76 | −351.81 | 154.3 | −13.19 |
per 1 mol of | −152.88 | −175.91 | 77.15 | −6.595 |
Changes in standard condition (2)
- Reaction of and sulfuric acid
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | – | – | 151.9 | −13.40 |
| – | – | 151.9 | −13.40 | |
per 1 mol of | – | – | 75.95 | −6.700 |
per 1 mol of | – | – | 151.9 | −13.40 |
per 1 mol of | – | – | 151.9 | −13.40 |
per 1 mol of | – | – | 75.95 | −6.700 |
Changes in standard condition (3)
- Reaction of and sulfuric acid◆
ΔrG −353.23 kJ/mol K 7.64 × 1061 pK −61.88
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −307.31 | −353.23 | 153.9 | −14.44 |
| −307.31 | −353.23 | 153.9 | −14.44 | |
per 1 mol of | −153.66 | −176.62 | 76.95 | −7.220 |
per 1 mol of | −307.31 | −353.23 | 153.9 | −14.44 |
per 1 mol of | −307.31 | −353.23 | 153.9 | −14.44 |
per 1 mol of | −153.66 | −176.62 | 76.95 | −7.220 |
Changes in aqueous solution (1)
- Reaction of and sulfuric acid◆
ΔrG −271.1 kJ/mol K 3.12 × 1047 pK −47.49
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −165.9 | −271.1 | 352.2 | – |
| −165.9 | −271.1 | 352.2 | – | |
per 1 mol of | −82.95 | −135.6 | 176.1 | – |
per 1 mol of | −165.9 | −271.1 | 352.2 | – |
per 1 mol of | −165.9 | −271.1 | 352.2 | – |
per 1 mol of | −82.95 | −135.6 | 176.1 | – |
Changes in aqueous solution (2)
- Reaction of and sulfuric acid◆
ΔrG −271.6 kJ/mol K 3.82 × 1047 pK −47.58
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −192.0 | −271.6 | 265.9 | – |
| −192.0 | −271.6 | 265.9 | – | |
per 1 mol of | −96.00 | −135.8 | 132.9 | – |
per 1 mol of | −192.0 | −271.6 | 265.9 | – |
per 1 mol of | −192.0 | −271.6 | 265.9 | – |
per 1 mol of | −96.00 | −135.8 | 132.9 | – |
Changes in aqueous solution (3)
- Reaction of and sulfuric acid◆
ΔrG −258.1 kJ/mol K 1.65 × 1045 pK −45.22
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −180.1 | −258.1 | 262.2 | 507 |
| −180.1 | −258.1 | 262.2 | 507 | |
per 1 mol of | −90.05 | −129.1 | 131.1 | 254 |
per 1 mol of | −180.1 | −258.1 | 262.2 | 507 |
per 1 mol of | −180.1 | −258.1 | 262.2 | 507 |
per 1 mol of | −90.05 | −129.1 | 131.1 | 254 |
Changes in aqueous solution (4)
- Reaction of and sulfuric acid◆
ΔrG −258.6 kJ/mol K 2.02 × 1045 pK −45.30
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −206.2 | −258.6 | 175.9 | – |
| −206.2 | −258.6 | 175.9 | – | |
per 1 mol of | −103.1 | −129.3 | 87.95 | – |
per 1 mol of | −206.2 | −258.6 | 175.9 | – |
per 1 mol of | −206.2 | −258.6 | 175.9 | – |
per 1 mol of | −103.1 | −129.3 | 87.95 | – |
Changes in aqueous solution (5)
- Reaction of and sulfuric acid◆
ΔrG −271.1 kJ/mol K 3.12 × 1047 pK −47.49
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −165.9 | −271.1 | 352.2 | – |
| −165.9 | −271.1 | 352.2 | – | |
per 1 mol of | −82.95 | −135.6 | 176.1 | – |
per 1 mol of | −165.9 | −271.1 | 352.2 | – |
per 1 mol of | −165.9 | −271.1 | 352.2 | – |
per 1 mol of | −82.95 | −135.6 | 176.1 | – |
Changes in aqueous solution (6)
- Reaction of and sulfuric acid◆
ΔrG −271.6 kJ/mol K 3.82 × 1047 pK −47.58
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −192.0 | −271.6 | 265.9 | – |
| −192.0 | −271.6 | 265.9 | – | |
per 1 mol of | −96.00 | −135.8 | 132.9 | – |
per 1 mol of | −192.0 | −271.6 | 265.9 | – |
per 1 mol of | −192.0 | −271.6 | 265.9 | – |
per 1 mol of | −96.00 | −135.8 | 132.9 | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| (cr) α | 0[1] | 0[1] | 32.01[1] | 26.32[1] |
| (cr) β | – | – | 34.39[1] | 26.53[1] |
| (cr) γ | 1.55[1] | 1.42[1] | 32.43[1] | 27.57[1] |
| (g) | 280.7[1] | 238.5[1] | 173.70[1] | 20.79[1] |
| H2SO4 (cr) | – | – | – | – |
| H2SO4 (l) | -813.989[1] | -690.003[1] | 156.904[1] | 138.91[1] |
| H2SO4 (ai) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
| H2SO4 (l) 1 hydrate | -1127.621[1] | -950.383[1] | 211.54[1] | 214.85[1] |
| H2SO4 (l) 2 hydrate | -1427.100[1] | -1199.650[1] | 276.40[1] | 260.83[1] |
| H2SO4 (l) 3 hydrate | -1720.402[1] | -1443.980[1] | 345.39[1] | 318.95[1] |
| H2SO4 (l) 4 hydrate | -2011.199[1] | -1685.863[1] | 414.59[1] | 382.21[1] |
| H2SO4 (l) 6.5 hydrate | -2733.256[1] | -2285.734[1] | 587.89[1] | 570.28[1] |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (ai):Ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| MnSO4 (cr) | -1065.25[1] | -957.36[1] | 112.1[1] | 100.50[1] |
| MnSO4 (ai) | -1130.1[1] | -972.7[1] | -53.6[1] | -243[1] |
| MnSO4 (ao) | -1115.9[1] | -985.7[1] | 36.4[1] | – |
| MnSO4 (cr) 1 hydrate α | -1376.5[1] | – | – | – |
| MnSO4 (cr) 1 hydrate β | -1348.1[1] | – | – | – |
| MnSO4 (cr) 4 hydrate | -2258.1[1] | – | – | – |
| MnSO4 (cr) 5 hydrate | -2553.1[1] | – | – | 326[1] |
| MnSO4 (cr) 7 hydrate | -3139.3[1] | – | – | – |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 32.01 J · K−1 · mol−1
- ^ Cp°, 26.32 J · K−1 · mol−1
- ^ S°, 34.39 J · K−1 · mol−1
- ^ Cp°, 26.53 J · K−1 · mol−1
- ^ ΔfH°, 1.55 kJ · mol−1
- ^ ΔfG°, 1.42 kJ · mol−1
- ^ S°, 32.43 J · K−1 · mol−1
- ^ Cp°, 27.57 J · K−1 · mol−1
- ^ ΔfH°, 280.7 kJ · mol−1
- ^ ΔfG°, 238.5 kJ · mol−1
- ^ S°, 173.70 J · K−1 · mol−1
- ^ Cp°, 20.79 J · K−1 · mol−1
- ^ ΔfH°, -813.989 kJ · mol−1
- ^ ΔfG°, -690.003 kJ · mol−1
- ^ S°, 156.904 J · K−1 · mol−1
- ^ Cp°, 138.91 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -1127.621 kJ · mol−1
- ^ ΔfG°, -950.383 kJ · mol−1
- ^ S°, 211.54 J · K−1 · mol−1
- ^ Cp°, 214.85 J · K−1 · mol−1
- ^ ΔfH°, -1427.100 kJ · mol−1
- ^ ΔfG°, -1199.650 kJ · mol−1
- ^ S°, 276.40 J · K−1 · mol−1
- ^ Cp°, 260.83 J · K−1 · mol−1
- ^ ΔfH°, -1720.402 kJ · mol−1
- ^ ΔfG°, -1443.980 kJ · mol−1
- ^ S°, 345.39 J · K−1 · mol−1
- ^ Cp°, 318.95 J · K−1 · mol−1
- ^ ΔfH°, -2011.199 kJ · mol−1
- ^ ΔfG°, -1685.863 kJ · mol−1
- ^ S°, 414.59 J · K−1 · mol−1
- ^ Cp°, 382.21 J · K−1 · mol−1
- ^ ΔfH°, -2733.256 kJ · mol−1
- ^ ΔfG°, -2285.734 kJ · mol−1
- ^ S°, 587.89 J · K−1 · mol−1
- ^ Cp°, 570.28 J · K−1 · mol−1
- ^ ΔfH°, -1065.25 kJ · mol−1
- ^ ΔfG°, -957.36 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 100.50 J · K−1 · mol−1
- ^ ΔfH°, -1130.1 kJ · mol−1
- ^ ΔfG°, -972.7 kJ · mol−1
- ^ S°, -53.6 J · K−1 · mol−1
- ^ Cp°, -243. J · K−1 · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfG°, -985.7 kJ · mol−1
- ^ S°, 36.4 J · K−1 · mol−1
- ^ ΔfH°, -1376.5 kJ · mol−1
- ^ ΔfH°, -1348.1 kJ · mol−1
- ^ ΔfH°, -2258.1 kJ · mol−1
- ^ ΔfH°, -2553.1 kJ · mol−1
- ^ Cp°, 326. J · K−1 · mol−1
- ^ ΔfH°, -3139.3 kJ · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1