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Answer :
Increasing the volume will shift the reaction to the right in the direction of products.
When the volume of a system at equilibrium is increased, according to Le Chatelier's principle, the system will shift in a way that reduces the pressure. In this particular reaction, increasing the volume will decrease the pressure.
As a result, the system will try to counteract this change by favoring the side with fewer moles of gas, which is the side of the reaction with fewer gas molecules. In this case, the products side has fewer gas molecules (1 mol of CO₂) compared to the reactants side (1 mol of CO). Therefore, the reaction will shift to the right, towards the products, in order to decrease the pressure.
Le Chatelier's principle states that a system at equilibrium will respond to any external changes or disturbances by shifting the equilibrium position in a way that minimizes the effect of those changes. One such external change is a variation in volume. When the volume of a system at equilibrium is increased, the pressure inside the system decreases. In order to counteract this decrease in pressure, the system will shift in the direction that produces more gas molecules, thus increasing the pressure.
In the given reaction, the reactants side contains one mole of CO gas, while the products side contains one mole of CO₂ gas. As a result, the products side has fewer gas molecules compared to the reactants side. By increasing the volume, the pressure will decrease, and the system will respond by shifting to the side with fewer gas molecules, which is the products side. Therefore, the reaction will shift to the right in the direction of products.
It's important to note that while increasing the volume favors the products in this reaction, the equilibrium constant (K) remains unchanged. The equilibrium constant only depends on temperature and is independent of any changes in concentration, pressure, or volume.
Learn more about Le Chatelier's principle
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