Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is increased by adding an inert gas (and everything else is held constant)? N2(g) + 3H2(g) Equilibrium arrow.jpg 2NH3(g) Group of answer choices To 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 adding an inert gas (and everything else is held constant)?
N2(g) + 3H2(g) Equilibrium arrow.jpg 2NH3(g)
Group of answer choices
To the left (more reactants)
To the right (more products)
It will not shift
Solution
The equilibrium will not shift.
Here's why:
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The reaction in question is N2(g) + 3H2(g) ⇌ 2NH3(g). This is an exothermic reaction, meaning it releases heat.
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When an inert gas is added to a system at equilibrium, the total pressure of the system increases. However, the partial pressures of the individual gases (N2, H2, and NH3 in this case) do not change because the inert gas does not react with any of them.
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According to Le Chatelier's Principle, a system at equilibrium will shift to counteract any change in conditions. However, since the partial pressures of the gases involved in the reaction do not change when an inert gas is added, the system does not "sense" any change and therefore does not shift.
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Therefore, the equilibrium will not shift to the left or the right when an inert gas is added to this system.
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