Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is increased by decreasing the volume (and everything else is held constant)?2SO2(g) + O2(g) 2SO3(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 increased by decreasing the volume (and everything else is held constant)?2SO2(g) + O2(g) 2SO3(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift
Solution
The equilibrium of an exothermic reaction will shift in response to changes in pressure due to Le Chatelier's Principle, which states that a system in equilibrium will adjust to minimize a change in conditions.
In the given reaction, 2SO2(g) + O2(g) ⇌ 2SO3(g), there are 3 moles of gas on the reactant side (2 moles of SO2 and 1 mole of O2) and 2 moles of gas on the product side (2 moles of SO3).
If the pressure is increased by decreasing the volume, the system will respond by shifting the equilibrium to the side with fewer moles of gas to counteract the increase in pressure. In this case, that is the product side (right side) of the equation.
So, the equilibrium will shift to the right (more products).
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