Highschool chemistry question on Le Chatlier's Principle

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SUMMARY

The discussion centers on Le Chatelier's Principle (LCP) as it applies to the chemical reaction A(aq) + B(aq) <-> C(aq). When the concentration of reactant A is increased, the system shifts to the right to form more product C, resulting in a higher concentration of A at the new equilibrium and a lower concentration of C. This behavior exemplifies LCP, which states that a system at equilibrium will adjust to counteract changes in concentration, temperature, or pressure.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with Le Chatelier's Principle
  • Basic knowledge of aqueous solutions
  • Ability to formulate and interpret equilibrium equations
NEXT STEPS
  • Study the mathematical formulation of equilibrium constants
  • Explore the impact of temperature changes on equilibrium
  • Learn about the effects of pressure changes on gaseous equilibria
  • Investigate real-world applications of Le Chatelier's Principle in industrial processes
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j3llzang
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Homework Statement


I just have a concept question on LCP.
in reaction: A(aq) + B(aq) <-> C(aq)
A is added and rxn is left to reach a new equilibrium.
Once @ new eqm, is [A] higher than before? and obviously [C] is lower, right?
 
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j3llzang said:

Homework Statement


I just have a concept question on LCP.
in reaction: A(aq) + B(aq) <-> C(aq)
A is added and rxn is left to reach a new equilibrium.
Once @ new eqm, is [A] higher than before? and obviously [C] is lower, right?

I hope you will get to a point where the opposite is obvious.

"Changing the concentration of an ingredient will shift the equilibrium to the side that would reduce that change in concentration. The chemical system will attempt to partially oppose the change affected to the original state of equilibrium."

http://en.wikipedia.org/wiki/Le_Chatelier's_principle

It will probably help if you can formulate the equations, equilibrium equations + conservation of mass and see what they tell you.
 

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