Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is decreased by increasing the volume (and everything else is held constant)?N2(g) + 3H2(g) 2NH3(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift
Question
Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is decreased by increasing the volume (and everything else is held constant)?N2(g) + 3H2(g) 2NH3(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift
Solution
The equilibrium of a reaction can shift based on changes in pressure, temperature, or concentration of reactants or products. This is described by Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
In the given reaction, N2(g) + 3H2(g) ⇌ 2NH3(g), there are 4 moles of gas on the reactant side (1 mole of N2 and 3 moles of H2) and 2 moles of gas on the product side (2 moles of NH3).
If the pressure is decreased by increasing the volume, the reaction will shift towards the side with more moles of gas to increase the pressure and counteract the change. In this case, that is the reactant side.
Therefore, the equilibrium will shift to the left (more reactants).
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