Le Chatelier's Principle Chemistry Example 3

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Example 3

medium
For the equilibrium CaCO3(s)⇌CaO(s)+CO2(g)\text{CaCO}_3\text{(s)} \rightleftharpoons \text{CaO(s)} + \text{CO}_2\text{(g)} (endothermic), predict the effect of increasing temperature on the amount of CO2\text{CO}_2 produced.

Solution

  1. 1
    The reaction is endothermic, meaning heat can be thought of as a 'reactant': heat+CaCO3⇌CaO+CO2\text{heat} + \text{CaCO}_3 \rightleftharpoons \text{CaO} + \text{CO}_2.
  2. 2
    Increasing temperature adds heat (a reactant), so the equilibrium shifts to the right, producing more CO2\text{CO}_2.

Answer

More CO2 is produced (equilibrium shifts right).\text{More CO}_2\text{ is produced (equilibrium shifts right).}
For endothermic reactions, increasing temperature shifts the equilibrium toward products. This is why calcium carbonate decomposes more readily at higher temperatures — the equilibrium favors lime (CaO) and carbon dioxide.

About Le Chatelier's Principle

When a system at chemical equilibrium is subjected to an external stress — such as a change in concentration, pressure, or temperature — the equilibrium.

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More Le Chatelier's Principle Examples

Example 1 easy

State Le Chatelier's principle and explain what it predicts about equilibrium systems.

Example 2 medium

For the exothermic reaction [formula], predict the effect of: (a) increasing temperature, (b) removi

Example 4 hard

The contact process produces sulfur trioxide: [formula], [formula]. Explain why the industrial proce

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