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I thought the rule for volume decrease is that the side with less moles will be favored; however, in 5.39 the volume was halved and the reactant which has more moles in equation, I calculated it to have increased in concentration.
Maia_Jackson_2C wrote:The rule is that the reaction will favor the side with less moles of gas for a volume decrease, you didn't mention gases so maybe the moles you counted weren't for gases?
This. Little details like these are the real kickers. Hope you figured it out OP.
This rule only applies when gases are present, if the system only has solids or liquids then a change in volume would not shift the equilibrium because compressing solids and liquids does not make them react more/less
PranaviKolla2B wrote:Can someone explain what it means when the reaction shifts one way or another?
A reaction shifts left when reactants are being produced at a higher rate than products and a reaction that shifts right means that products are being formed at a higher rate than the reactants.
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