Which way will the equilibrium shift, for the exothermic reaction below, if additional SO3(g) is added (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 additional SO3(g) is added (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 a reaction can be shifted by changing the conditions that the reaction is under. 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 moves to counteract the change.
In the given reaction, 2SO2(g) + O2(g) ⇌ 2SO3(g), SO3 is a product. If we add more SO3 to the system, we are increasing the concentration of the product.
According to Le Chatelier's Principle, the system will try to counteract this change by shifting the equilibrium to the left to consume some of the added SO3. This shift to the left means the reaction will produce more reactants (SO2 and O2).
So, the answer is: To the left (more reactants).
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