Which way will the equilibrium shift, for the exothermic reaction below, if additional NH3(g) is added (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 additional NH3(g) is added (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 be predicted using 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, N2(g) + 3H2(g) ⇌ 2NH3(g), the production of NH3(g) is exothermic. This means that heat is a product of the reaction.
If additional NH3(g) is added to the system, the system will try to counteract this change by reducing the amount of NH3(g). It can do this by shifting the equilibrium to the left, towards the reactants, N2(g) and H2(g).
So, the equilibrium will shift to the left (more reactants).
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