Practice Le Chatelier's Principle in Chemistry
Use these practice problems to test your method after reviewing the concept explanation and worked examples.
Quick Recap
When a system at equilibrium is disturbed, it shifts to counteract the disturbance.
Push on equilibrium, and it pushes back. Add something, and the system uses it up.
Example 1
easyState Le Chatelier's principle and explain what it predicts about equilibrium systems.
Example 2
mediumFor the exothermic reaction \text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3 + \text{heat}, predict the effect of: (a) increasing temperature, (b) removing \text{NH}_3, (c) increasing pressure.
Example 3
mediumFor the equilibrium \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 \text{CO}_2 produced.
Example 4
hardThe contact process produces sulfur trioxide: 2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{SO}_3\text{(g)}, \Delta H = -198\,\text{kJ}. Explain why the industrial process uses: (a) high pressure, (b) moderate temperature (450°\text{C}) rather than low temperature, and (c) a \text{V}_2\text{O}_5 catalyst.