For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.
a. C(s) + H₂O(g) ⇌ CO(g) + H₂(g)

Question

For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.

a. C(s) + H₂O(g) ⇌ CO(g) + H₂(g)

Accepted Answer

Welcome back, everyone predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture. Using Leat Lia's principle, we've got two moles of phosphorus Penta solid reacting with oxygen gas and equilibrium with the products, two moles of phosphorus oxy chloride gas, and two moles of chlorine gas. And then we have choices A through D which predict the shifts in equilibrium either in a forward or backward reaction and either favoring formation of reactants or products. So let's start by recalling that what Lelia's principle is useful for is to describe how equilibrium responds to changes in temperature concentration or pressure. And in the same way, volume recall that according to Boyle's law, pressure is inversely proportional to volume. So if pressure is increasing, then volume is decreasing. And this is true when the moles of our substance and temperature are constant. So it's derived from our IDL gas law PV equals N RT and that is what is occurring here. So looking at our reaction, we're going to need to determine the moles of gas on each side of the reaction. On the reactant side, we have just one mole of oxygen gas. So we have one mole of gas on the reactant side. And then on the product side, we have two, we have a total of four moles of gaseous products. So that's four moles of gas. If the pressure is increased by decreasing the volume of this reaction. Recall that gaseous substances or gaseous molecules, the fewer of them that we have, then the lower occupied volume by these molecules. And that will correspond to an exertion of less pressure on the system. And so, if again, pressure is increased by decreasing the volume, then equilibrium will want to shift in the direction where there is less gaseous molecules exerting less pressure overall on the system. And so equilibrium, we would want to draw the half arrow going a longer direction towards the right for the formation of more reactants based on our answer choices, we would rule out choice A which says that the reaction will shift forward, favoring formation of the reactants where the reactants are on the left hand side of the equilibrium arrow. So we would rule out choice A for that reason. Then choice B, we can place a check mark by because it does agree with the fact that the reaction should shift backward and favor formation of the reactants, which is what we outlined. Choice C we can rule out because again, it says that the reaction should shift forward, favoring formation of the products which we disagreed with. And choice D states that the will shift backward and favor formation of the products which again is untrue. So that means that B is our final answer to complete this example that when pressure is increased by decreasing the volume of an equilibrium mixture, using leat principle, we would suggest that equilibrium or we would agree that equilibrium would shift towards the left in favor of formation of more reactants. Since there are less gaseous molecules on the reactant side, occupying less volume and exerting less pressure. So again, our answer is choice B I hope this made sense and let us know if you have any questions.

For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.
a. C(s) + H₂O(g) ⇌ CO(g) + H₂(g)

Verified video answer for a similar problem:

Key Concepts

Le Châtelier's Principle

Equilibrium and Reaction Quotient

Effect of Pressure on Gaseous Reactions

For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture. a. C(s) + H2O(g) ⇌ CO(g) + H2(g)

Verified video answer for a similar problem:

Key Concepts

Le Châtelier's Principle

Equilibrium and Reaction Quotient

Effect of Pressure on Gaseous Reactions

For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.
a. C(s) + H₂O(g) ⇌ CO(g) + H₂(g)