Home › AP Chemistry › Chemistry › Fundamental Equilibrium Concepts › Removing hydrogen iodide from its equilibrium mi…
Removing hydrogen iodide from its equilibrium mixture leaves the concentrations of all three species:
ALower than before
BHigher than before
CExactly unchanged
DImpossible to predict
Answer & Solution
Correct answer: A. Lower than before
1. Different ways of stressing the same equilibrium give different final compositions.
2. The three different ways of inducing this stress result in three different changes in the composition of the equilibrium mixture.
3. If hydrogen iodide is removed, the concentrations of all three species will be lower when equilibrium is reestablished.
4. The system rebuilds some product but never recovers what was taken.
_Source: OpenStax Chemistry 2e (CC BY 4.0), Ch 13 'Fundamental Equilibrium Concepts', sections 13.1-13.4_
Related questions
The reaction quotient is useful during a reaction because its value:Many real systems involve coupled equilibria, meaning two reactions that share:Adding 0.10 mol of nitrogen dioxide to a 1.0 litre flask at 25 degrees Celsius left equiliReactions differ from many physical processes in that they may proceed:A reaction quotient equation using absolute concentrations rather than relative values is:Changing the volume of a gas-phase equilibrium changes the concentrations of:Multiplying every stoichiometric coefficient in an equation by a factor changes K:Adding hydrogen or iodine to a hydrogen iodide equilibrium increases the rate of: