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Le Chatelier's Principle Reaction

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(1) Using Le Chatelier's principle, indicate how each change will affect the following reactions. Justify your answer.

2NaOH(aq) + CO2(g) <---> Na2CO3(aq) + H2O(l) delta H = -180kJ/mol

(a) Removing Na2CO3 from the reaction vessel.
(b) Adding more CO2(g) thereby increasing the pressure in the reaction vessel. Consider both the addition of reagent and the change in pressure in your answer.
(c) Adding an inert gas to the reaction mixture to increase the pressure in the reaction vessel.
(d) Lowering the temperature of the reaction vessel.

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Solution Preview

a. Aqueous Na2CO3 is a product. If it is removed, then to come back to equilibrium, more product must form. Hence, removing Na2CO3 will result in the formation of even more Na2CO3.

b. In terms of reagent, adding more reactant increases reactant concentration initially. To counter this increase, more product must form. Hence, in terms of adding more reagent, the equilibrium will shift to the right resulting in more ...

Solution Summary

The expert examines Le Chatelier's principles in a reaction. The reaction vessels for removing Na2CO3 are determined.