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NEETChemistryChemical Equilibrium

Consider the exothermic oxidation of sulfur dioxide at equilibrium: 2 SO ₂( g ) + O ₂( g ) 2 SO ₃( g ) + Heat Which of the following actions will decrease the equilibrium yield of SO ₃ ?

Options

  1. ADecreasing the temperature
  2. BIncreasing the pressure
  3. CAdding an inert gas at constant volume
  4. DAdding an inert gas at constant pressure

Correct answer

D. Adding an inert gas at constant pressure

Step-by-step solution

The given reaction is exothermic. According to Le Chatelier's principle, decreasing the temperature will shift the equilibrium in the forward direction, increasing the yield of SO ₃ . The number of gaseous moles on the reactant side is 2 + 1 = 3 , and on the product side is 2 . Since n_g = 2 - 3 = -1 , increasing the pressure will shift the equilibrium towards the side with fewer gaseous moles (forward direction), increasing the yield of SO ₃ . Adding an inert gas at constant volume does not change the partial pres

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