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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.

    © BrainMass Inc. brainmass.com December 24, 2021, 11:11 pm ad1c9bdddf
    https://brainmass.com/chemistry/le-chatelier-s-principle/le-chateliers-principle-reaction-546199

    SOLUTION This solution is FREE courtesy of BrainMass!

    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 product formation.
    In terms of pressure, adding more gaseous CO2 increases the pressure. To counter this increase, the equilibrium will shift to the direction that results in lower pressure. Lower pressure comes from less gaseous molecules. The side that has less gaseous molecules is the product side. Hence, shifting to the products side will result in alleviating the pressure increase which means more product will form.

    c. Adding an inert gas will not shift the equilibrium to either side as long as volume is constant. This is because the partial pressure of each gas remains the same as concentration is same under constant volume conditions, so it's as if the amounts of reactant and product are unchanged. When amounts of both reactant and product are not changed, the equilibrium will not shift.

    d. The reaction is exothermic as dH is negative. Hence, heat is released as a product in this reaction. Lowering the temperature is equivalent to removing heat from the system. As heat is a product, by lowering temperature we are removing product. If product is removed, product concentration is decreased. To counter this decrease, more product should form to come back to equilibrium. Hence, the reaction will shift to products side resulting in more product being formed.

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    © BrainMass Inc. brainmass.com December 24, 2021, 11:11 pm ad1c9bdddf>
    https://brainmass.com/chemistry/le-chatelier-s-principle/le-chateliers-principle-reaction-546199

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