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Reversible reactions and equilibrium
Recognize that certain chemical reactions can reverse, indicated by the symbol ⇌.
11
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110
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77
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90 min
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CambridgeIGCSEChemistryChemical reactions
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Reversible reactions and equilibrium outcomes11 objectives
- Recognize that certain chemical reactions can reverse, indicated by the symbol ⇌.
- Explain how altering conditions can influence the direction of a reversible reaction, specifically regarding: (a) the impact of heat on hydrated substances (b) the effect of adding water to anhydrous substances, limited to copper(II) sulfate and cobalt(II) chloride.
- Identify that a reversible reaction in a closed system reaches equilibrium when: (a) the rate of the forward reaction matches the rate of the reverse reaction (b) the concentrations of reactants and products remain constant.
- Anticipate and clarify how the position of equilibrium in a reversible reaction is influenced by: (a) temperature changes (b) pressure changes (c) concentration changes (d) the introduction of a catalyst, based on provided information.
- Write the symbol equation for ammonia production in the Haber process: N₂(g) + 3H₂(g) ⇌ 2NH₃(g).
- Identify the sources of hydrogen (from methane) and nitrogen (from air) used in the Haber process.
- Specify the typical conditions for the Haber process, which are 450 °C, 20,000 kPa (200 atm), and the use of an iron catalyst.
- Write the symbol equation for the conversion of sulfur dioxide to sulfur trioxide in the Contact process: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g).
- Identify the sources of sulfur dioxide (from burning sulfur or roasting sulfide ores) and oxygen (from air) in the Contact process.
- Specify the typical conditions for converting sulfur dioxide to sulfur trioxide in the Contact process, which are 450 °C, 200 kPa (2 atm), and the use of vanadium(V) oxide as a catalyst.
- Discuss, in terms of reaction rates and equilibrium position, the rationale behind the typical conditions used in both the Haber process and the Contact process, considering safety and economic factors.
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