Match the change in reaction condition with its effect on the equilibrium of a reversible reaction: Increase in Pressure (for gaseous reactions) Increase in Product Concentration I... Match the change in reaction condition with its effect on the equilibrium of a reversible reaction: Increase in Pressure (for gaseous reactions) Increase in Product Concentration Increase in Reactant Concentration
Understand the Problem
The question asks to match changes in reaction conditions (pressure, product concentration, reactant concentration) with their effects on the equilibrium of a reversible reaction. This relates to Le Chatelier's principle, which states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.
Answer
* Increase in Pressure (gaseous reactions): Shifts to fewer gas moles. * Increase in Product Concentration: Shifts to reactants. * Increase in Reactant Concentration: Shifts to products.
Here's how changes in reaction conditions affect equilibrium:
- Increase in Pressure (gaseous reactions): Shifts equilibrium towards the side with fewer moles of gas.
- Increase in Product Concentration: Shifts equilibrium towards reactants.
- Increase in Reactant Concentration: Shifts equilibrium towards products.
Answer for screen readers
Here's how changes in reaction conditions affect equilibrium:
- Increase in Pressure (gaseous reactions): Shifts equilibrium towards the side with fewer moles of gas.
- Increase in Product Concentration: Shifts equilibrium towards reactants.
- Increase in Reactant Concentration: Shifts equilibrium towards products.
More Information
Le Chatelier's principle is a key concept here, stating that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress. Changes in concentration, pressure, or temperature can affect the equilibrium position.
Tips
A common mistake is to forget that pressure changes only significantly affect gaseous reactions where there's a difference in the number of moles of gas on each side of the equation.
Sources
- Le Chatelier's Principle Fundamentals - Chemistry LibreTexts - chem.libretexts.org
- The Effect of Changing Conditions - Chemistry LibreTexts - chem.libretexts.org
- Increasing the concentration of a reactant shifts the position of ... - Vaia - vaia.com
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