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)? H2(g) + I2(g) Equilibrium arrow.jpg 2HI(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)?
H2(g) + I2(g) Equilibrium arrow.jpg 2HI(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: H2(g) + I2(g) ⇌ 2HI(g). This is an exothermic reaction, meaning it releases heat.
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According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in pressure, temperature, or concentration of components, the system will shift its equilibrium position to counteract the effect of the disturbance.
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In this case, the pressure is increased by adding an inert gas. An inert gas does not react with any of the components in the system. Therefore, it does not change the partial pressures of the reactants or products.
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Since the partial pressures of the reactants and products are not changed, the position of the equilibrium does not shift.
So, the answer is "It will not shift".
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