Decomposition of Sodium Bicarbonate

2NaHCO₃ → Na₂CO₃ + H₂O + CO₂

Descripción general

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.

Participantes

Rol	Sustancia	Coeficiente	Estado
Reactivo	Sodium Bicarbonate NaHCO₃	2	(s)
Producto	Sodium Carbonate Na₂CO₃	1	(s)
Producto	Water H₂O	1	(g)
Producto	Carbon Dioxide CO₂	1	(g)

Ejemplo cotidiano

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.

Importancia industrial

Esta reacción es fundamental para la industria de la panadería. El bicarbonato de sodio también se utiliza en extintores, donde el CO₂ liberado ayuda a sofocar las llamas.

Propiedades

Tipo: Decomposition
Reversible: No
Energía: Endotérmico
ΔH: 129,0 kJ/mol

Reacciones relacionadas

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.