Which way will the equilibrium shift, for the endothermic reaction below, if the pressure is increased by decreasing the volume (and everything else is held constant)?N2O4(g) 2NO2(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 endothermic reaction below, if the pressure is increased by decreasing the volume (and everything else is held constant)?N2O4(g) 2NO2(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 Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
In the given reaction, N2O4(g) ⇌ 2NO2(g), there are fewer moles of gas on the reactant side (1 mole of N2O4) than on the product side (2 moles of NO2).
When the pressure is increased by decreasing the volume, the equilibrium will shift to the side with fewer moles of gas to counteract the change and decrease the pressure.
Therefore, for this endothermic reaction, if the pressure is increased by decreasing the volume (and everything else is held constant), the equilibrium will shift to the left (more reactants).
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