Which of the following gaseous reactions would be favoured...

Which of the following gaseous reactions would be favoured by reducing the pressure (a) $\mathrm{PCl}_{5} \Rightarrow \mathrm{PCl}_{3}+\mathrm{Cl}_{2}$ (b) $2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}$ (c) $\mathrm{PCl}_{3}+\mathrm{Cl}_{2}=\mathrm{PCl}_{3}$ (d) $\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$

Which of the following gaseous reactions would be favoured by reducing the pressure
(a) $\mathrm{PCl}_{5} \Rightarrow \mathrm{PCl}_{3}+\mathrm{Cl}_{2}$
(b) $2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}$
(c) $\mathrm{PCl}_{3}+\mathrm{Cl}_{2}=\mathrm{PCl}_{3}$
(d) $\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Stoichiometry and Mole Counting in Gaseous Reactions

Determining the number of gaseous moles on each side of a chemical equation is essential when predicting the impact of pressure changes. By comparing the total moles of gas in the reactants and products, one can predict the direction in which the equilibrium will shift when pressure is altered, based on the principles of equilibrium dynamics.

Le Chatelier's Principle

This principle explains that if a system at equilibrium experiences a change in conditions, such as pressure, temperature, or concentration, the system will adjust its equilibrium position to counteract that change. In the context of gaseous reactions, it means that the reaction will shift in a direction that tends to minimize the impact of the imposed pressure change.

Effect of Pressure Changes on Gaseous Equilibrium

In gas-phase reactions, pressure is directly related to the concentration of gas molecules. When the pressure is reduced, the equilibrium shifts toward the side of the reaction with a greater number of gas molecules because this shift helps to increase the pressure back toward its original state. Conversely, increasing the pressure favors the side with fewer gas molecules.

Transcript

Please give Ace some feedback