Decomposition of Sodium Bicarbonate

2NaHCO3 → Na2CO3 + H2O + CO2

Aperçu

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

Rôle Substance Coefficient État
Réactif Sodium Bicarbonate NaHCO₃ 2 (s)
Produit Sodium Carbonate Na₂CO₃ 1 (s)
Produit Water H₂O 1 (g)
Produit Carbon Dioxide CO₂ 1 (g)

Exemple du quotidien

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.

Importance industrielle

This reaction is fundamental to the baking industry. Sodium bicarbonate is also used in fire extinguishers, where the CO2 released helps smother flames.

Propriétés

Type
Decomposition
Réversible
Non
Énergie
Endothermique
ΔH
129,0 kJ/mol

Réactions associées

Decomposition of Ammonium Nitrate Decomposition of Calcium Hypochlorite Decomposition of Carbonic Acid Decomposition of Iron(II,III) Oxide (Direct Reduction) Decomposition of Nitrous Oxide (Laughing Gas) Decomposition of Barium Peroxide Decomposition of Water (Electrolysis) Thermal Decomposition of Copper(II) Carbonate Thermal Decomposition of Mercury(II) Oxide Cracking of Octane (Thermal Cracking)

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.