According to Le Chatelier’s principle, which direction will the equilibrium shift if the concentration...?

According to Le Chatelier’s principle, which direction will the equilibrium shift if the concentration of the H2C2O4 is increased according to this reaction at equilibrium:
2Ce(IO3)4(aq) + 24 H2C2O4(aq) —> Ce2(C2O4)3(aq) + 4I2(aq) + 42 CO2(g) + 24 H2O(l)

Answer:
These questions are misleading. The best you can ever do is to have a stoichometric amount of each reactant. Any deviation from this will actually lead to PROPORTIONATELY less product being formed.
LeChatlier's principle says that if you increase the concentration of a reactant, the equilibrium will shift to use up some of that reactant. In this case, the equilibrium will shift to the right, increasing the concentrations of all of the products.
According to Le Chatelier's principle, if a stress is applied to a system, the system will shift in order to reestablish equilibrium. For the equation, since H2C2O4 (in the left side of equation) is increased, then the equilibrium will shift to the right to make up for the increase in H2C2O4.

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