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CHEM105 Study Guide - Final Guide: Reaction Quotient, Inert Gas, Equilibrium Constant

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Yoram Apelblat
Study Guide

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Chemical Equilibrium
All reactions will reach a state of equilibrium
Both the products and the reactants are present and their concentration
does not seem to be changing
o Reaction is occurring microscopically only
o Rate of products formed equals the rate of reactants consumed
Equilibrium constant
  
 
measures the extent of the reaction
o K is constant only if temperature is constant
o Small K yields little product
o Large K goes to completion
      
o Solids and liquids do not appear in the equilibrium expression
If rxn3 = rxn1 + rxn2, then K3 = K1K2
Reaction quotient
Similar to K but all the concentrations are taken at another point in the
Reaction quotient (Q) is compared to K to see which direction the
reaction will proceed in
o Q < K, too much reactant, not enough product, rxn goes ->
o Q > K, not enough reactant, too much product, rxn goes <-
o Q = K, reaction is at equilibrium
Le Chatelier’s principle
If a change is imposed on a system at equilibrium, the position of the
equilibrium will shift in the direction that reduce the change.
Changes in concentration
o Reaction will go in the direction that restores concentration
Adding/removing reactants/products
o Equilibrium will shift such that the concentration of that
component is restored
Pressure change
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