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Chapter 14: Problem 7

In the context of Le Chatelier's principle, what is a "stress"? List the stresses that affect chemical equilibria.

Short Answer

Expert verified
In the context of Le Chatelier's principle, a 'stress' is a disturbance or change to the equilibrium conditions (concentration, temperature, pressure/volume) of a chemical system. The reaction will shift to counteract this change or 'stress'.

Step by step solution

01

Defining 'Stress'

In the context of Le Chatelier's principle, a 'stress' refers to a change in conditions that can disrupt the equilibrium of a chemical system. Any change to the system's temperature, pressure, concentration or volume, can be considered a stress.
02

Listing the Stresses - Concentration

Changes in concentration can affect the chemical equilibrium. If the concentration of a reactant is increased, the reaction will move in the direction that uses up the added reactant (to the products side). Conversely, if the concentration of a product is increased, the reaction will move in the direction that uses up the added product (to the reactants side).
03

Listing the Stresses - Temperature

Changes in temperature can also stress a system. If heat is added to a system, the reaction will shift in the direction that absorbs the heat (endothermic direction). Conversely, if the system is cooled, the reaction will shift in the direction that releases heat (exothermic direction).
04

Listing the Stresses - Pressure and Volume

Changes in pressure and/or volume can affect a system at equilibrium as well. If pressure is increased (by decreasing volume) the reaction will move in the direction of fewer gas molecules. If pressure is decreased (by increasing volume), the reaction will move in the direction of more gas molecules. This is particularly applicable to gas-phase reactions.

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Most popular questions from this chapter

Changes in the concentrations of the reactants and products at equilibrium have no effect on the value of the equilibrium constant. Explain this statement.

Write the solubility product expressions for the following slightly soluble salts: AgI, \(\mathrm{SrSO}_{4}, \mathrm{Ag}_{2} \mathrm{CO}_{3}, \mathrm{Ag}_{2} \mathrm{S}, \mathrm{PbI}_{2}, \mathrm{AgIO}_{3}\) \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2},\) and \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\)

The solubility of cobalt \((\mathrm{II})\) sulfide, coS, is \(1.7 \times 10^{-13} \mathrm{M}\) . Calculate the solubility product constant for \(\mathrm{CoS} .\)

How would you explain Le Chatelier's principle in your own words to someone who finds the concept difficult to understand?

Explain the meaning of the terms reversible reaction, completion reaction, and reaction at equilibrium.
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