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Chapter 14: Problem 47

When does a pressure change affect a chemical equilibrium?

Short Answer

Expert verified
A pressure change affects a chemical equilibrium when there's a difference in the number of moles of gas between the reactants and products. With increased pressure, the equilibrium shifts towards the side of the reaction with fewer gaseous moles, and when pressure is decreased, it shifts towards the side with more gaseous moles.

Step by step solution

01

Understanding Pressure and its Effects on Equilibrium

Pressure does not directly affect the equilibrium constant, but it influences the composition of the equilibrium mixture, a concept that is observed with the help of Le Chatelier's principle. According to this principle, if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract and reestablish the equilibrium state.
02

Role of Volume and Pressure

Changes in pressure can also be seen as changes in volume. This is because pressure and volume are inversely proportional (according to Boyle's law). If the pressure is increased (or the volume is decreased), the equilibrium will shift to relieve that pressure by favoring the side of the reaction with fewer moles of gas.
03

Differences in Moles of Gaseous Reactants and Products

If the number of moles of gas is the same on both sides of the equation, there won't be a shift due to a change in pressure. However, if the number of moles of gas differs between the reactants and products, a change in pressure will cause a shift in the position of equilibrium. When pressure is increased, the equilibrium shifts towards the side of the reaction with fewer gaseous moles. Conversely, when the pressure is reduced, it shifts towards the side of the reaction with more gaseous moles.

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