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Can someone explain the Le Chatelier's principle please? Does concentration and partial pressure have the same effect on the reaction? For example, in problem 11.69 a) why does increasing the partial pressure of the reactant CO2 result in creation of more reactants and thus decrease the partial pressure of H2? While in part b, why does reducing the pressure of the product CO lead to the formation of more CO and the decrease in pressure of CO2? I thought by reducing the pressure of product will increase the pressure of the reactant in order to maintain equilibrium.
As a general rule, when you decrease the volume and thus increase the pressure under which the reaction is taking place, the reaction will favor the side with less moles of gas. If the pressure is increased and the product side of the reaction has less moles of gas, the reaction will favor the products, but if the reactant side has less moles of gas the reaction will favor the reactants.
Le Chatelier's principle states that if something disturbs the equilibrium, the positions of equilibrium will shift to counteract the change and re-establish the equilibrium So for example if in A + B <-> C +D if the concentration of A is increased than the equilibrium positions will shift and more A will interact with B thus creating more C and D and B and A will decrease so that the system re establishes the equilibrium. For pressure, increasing pressure will cause the the equilibrium to shift to the side with less moles because this will decrease the pressure and when decreasing pressure the equilibrium will shift to the side with more moles so that the pressure increases and retains equilibrium.
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