According to Le Chatelier's Principle, which perturbation will shift the equilibrium position of the exothermic Haber reaction toward product formation?
Answer and explanation
Correct answer: C. Increasing the total system pressure
- Step 1: Analyze moles of gas: Reactants have of gas, while products have of gas.
- Step 2: Evaluate pressure effect: An increase in total system pressure drives the equilibrium toward the side with fewer gas moles (the forward direction, producing ).
- Step 3: Verify temperature effect: Because the forward reaction is exothermic, increasing temperature shifts equilibrium toward reactants (backward).
Answer
Increasing the total system pressure.
Why not the others: 'Increasing temperature' shifts the exothermic equilibrium left; 'Decreasing nitrogen' removes a reactant and shifts left; 'Adding inert gas at constant volume' does not alter partial pressures or equilibrium position.
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