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Chem Chemistry

ChemistryNEB 2074 (old course) (grade increment)

What is the effect of increase of pressure and decrease of temperature in the following chemical equilibrium ? 2SO2 (g) + O2 (g) <= 2SO3 (g) + heat

2

Answer

· Based on the official syllabus and past papers
Updated

The given reaction is an exothermic reaction where the forward reaction is favoured by the application of pressure and lowering of temperature.

Effect of Increase of Pressure:

  • The reaction involves 3 moles of gaseous reactants and 2 moles of gaseous products.
  • According to Le Chatelier’s principle, increasing the pressure shifts the equilibrium in the direction where the number of moles of gas decreases.
  • Thus, the equilibrium shifts to the right, producing more .
00.751.52.253Reactants (3 moles gas)3Products (2 moles gas)2Total moles of gas
Pressure effect: Fewer gas moles favor forward reaction (2SO₂ + O₂ → 2SO₃)
22SO₂+O₂Pressure ↑Moles of gas: 3 → 222SO₃
Effect of increasing pressure: fewer moles of gas → equilibrium shifts right (2SO₂ + O₂ → 2SO₃)

Effect of Decrease of Temperature:

  • The reaction is exothermic, meaning heat is released during the forward reaction.
  • Lowering the temperature removes heat from the system, and the equilibrium shifts in the direction that produces heat.
  • Hence, the equilibrium shifts to the right, producing more .
22SO₂+O₂Temperature ↓Shift: ← (endothermic) → (exothermic)22SO₃
Effect of decreasing temperature on exothermic equilibrium (2SO₂ + O₂ ⇌ 2SO₃ + heat)

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