2Mg(HCO3)2 + Na2Cr2O7 💧→ 2MgCO3↓ + 2NaHCO3 + H2Cr2O7
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The reaction of magnesium hydrogencarbonate and sodium dichromate yields magnesium carbonate, sodium hydrogencarbonate, and dichromic acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of magnesium hydrogencarbonate and sodium dichromate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of magnesium hydrogencarbonate and sodium dichromate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Mg(HCO3)2 | Magnesium hydrogencarbonate | 2 | Lewis acid | Soluble in water |
Na2Cr2O7 | Sodium dichromate | 1 | Lewis base | Very soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgCO3 | Magnesium carbonate | 2 | Lewis conjugate | Very slightly soluble in water |
NaHCO3 | Sodium hydrogencarbonate | 2 | Non-redox product | – |
H2Cr2O7 | Dichromic acid | 1 | Non-redox product | – |
Thermodynamic changes
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 |
---|---|---|---|---|
Mg(HCO3)2 | – | – | – | – |
Na2Cr2O7 (cr) | -1978.6[1] | – | – | – |
Na2Cr2O7 (ai) | -1970.7[1] | -1824.9[1] | 379.9[1] | – |
Na2Cr2O7 (cr) 2 hydrate | -2574.8[1] | – | – | – |
* (cr):Crystalline solid, (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 |
---|---|---|---|---|
MgCO3 (cr) | -1095.8[1] | -1012.1[1] | 65.7[1] | 75.52[1] |
MgCO3 (cr) 3 hydrate | – | -1726.1[1] | – | – |
MgCO3 (cr) 5 hydrate | – | -2199.2[1] | – | – |
NaHCO3 (cr) | -950.81[1] | -851.0[1] | 101.7[1] | 87.61[1] |
NaHCO3 (ai) | -932.11[1] | -848.66[1] | 150.2[1] | – |
NaHCO3 (ao) | -943.9[1] | -849.7[1] | 113.8[1] | – |
H2Cr2O7 | – | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
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°, -1978.6 kJ · mol−1
- ^ ΔfH°, -1970.7 kJ · mol−1
- ^ ΔfG°, -1824.9 kJ · mol−1
- ^ S°, 379.9 J · K−1 · mol−1
- ^ ΔfH°, -2574.8 kJ · mol−1
- ^ ΔfH°, -1095.8 kJ · mol−1
- ^ ΔfG°, -1012.1 kJ · mol−1
- ^ S°, 65.7 J · K−1 · mol−1
- ^ Cp°, 75.52 J · K−1 · mol−1
- ^ ΔfG°, -1726.1 kJ · mol−1
- ^ ΔfG°, -2199.2 kJ · mol−1
- ^ ΔfH°, -950.81 kJ · mol−1
- ^ ΔfG°, -851.0 kJ · mol−1
- ^ S°, 101.7 J · K−1 · mol−1
- ^ Cp°, 87.61 J · K−1 · mol−1
- ^ ΔfH°, -932.11 kJ · mol−1
- ^ ΔfG°, -848.66 kJ · mol−1
- ^ S°, 150.2 J · K−1 · mol−1
- ^ ΔfH°, -943.9 kJ · mol−1
- ^ ΔfG°, -849.7 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1