Decomposition of Sodium Bicarbonate
2NaHCO3 → Na2CO3 + H2O + CO2
Overview
Sodium bicarbonate (baking soda) decomposes when heated above 50 C into sodium carbonate, water, and carbon dioxide. This thermal decomposition is the key reaction in baking, where the released CO2 gas creates the bubbles that make baked goods rise.
Participants
| Role | Substance | Coefficient | State |
|---|---|---|---|
| Reactant | Sodium Bicarbonate NaHCO₃ | 2 | (s) |
| Product | Sodium Carbonate Na₂CO₃ | 1 | (s) |
| Product | Water H₂O | 1 | (g) |
| Product | Carbon Dioxide CO₂ | 1 | (g) |
Everyday Example
When baking soda is added to cake batter and heated in the oven, this decomposition releases CO2 bubbles that make the cake fluffy and light.
Industrial Importance
This reaction is fundamental to the baking industry. Sodium bicarbonate is also used in fire extinguishers, where the CO2 released helps smother flames.
Properties
- Type
- Decomposition
- Reversible
- No
- Energy
- Endothermic
- ΔH
- 129.0 kJ/mol
Related Reactions
Cracking of Octane (Thermal Cracking)
Decomposition of Ammonium Nitrate
Decomposition of Barium Peroxide
Decomposition of Calcium Carbonate (Calcination)
Decomposition of Calcium Hypochlorite
Decomposition of Carbonic Acid
Decomposition of Hydrogen Peroxide
Decomposition of Iron(II,III) Oxide (Direct Reduction)
Decomposition of Nitroglycerin
Decomposition of Nitrous Oxide (Laughing Gas)
Frequently Asked Questions
What is the equation for Decomposition of Sodium Bicarbonate?
The balanced equation is: 2NaHCO₃ → Na₂CO₃ + H₂O + CO₂.
What type of reaction is Decomposition of Sodium Bicarbonate?
Decomposition of Sodium Bicarbonate is a decomposition reaction.
Is Decomposition of Sodium Bicarbonate exothermic or endothermic?
Decomposition of Sodium Bicarbonate is endothermic (absorbs energy). The enthalpy change (ΔH) is 129.0 kJ/mol.