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Equilibrium and Le Chateliers Principle

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1. Describe how temperature and concentration affect the equillibrium of a chemical system.

2. Apply Le Chatelier's Principle to predict the direction that a reaction will proceed given a particular set of conditions.

3. Explain the construction of equillibrium expressions in a general way.

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1. Describe how temperature and concentration affect the equillibrium of a chemical system.
Increasing the temperature of an exothermic reaction (where the heat term is on the right) will drive the equilibrium to the left whereas increasing the temperature of an endothermic reaction (where the heat term is on the left) will drive the equilibrium to the right.
Similarly, if we increase the concentration of any chemical species in a reaction, the equilibrium will shift away from that compound. In the following,
A + B <-------> C + D
if we increase the ...

Solution Summary

This solution provides explanations and calculations for equilibrium calculations.

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See Also This Related BrainMass Solution

Le Chateliers Principle

I already know what Le Chatliers Principle is, but I need help describing what is going on in specific in the following reactions. For example, how is the chemical equation changing to minimize change.

1. Bromine water is initially yellow/brown but changes to yellow when sodium hydroxide is added. Then when sulfuric acid is added the solution turns yellow/brown again.
What is happening? Note: Br2(aq) + H2O(l) <----> HOBr2(aq) + Br2 -(aq) + H+

2. Potassium chromate is initially yellow. When sulfuric acid is added the solution turns orange. Then when sodium hydroxide is added the solution turned back yellow.
What is happening? Note: CrO4 2-(aq) + 2H+(aq) <-----> Cr2O7 2-(aq) + H2O(aq)

3. Ethyl acetoacetate and water are clear initially, then when iron(III) chloride is added the solution turned deep purple. Then when bromine water was added the solution turned clear. Over time the deep purple color reappeared in the solution.
What is happening? Note: Ethyl acetate exists as an equilibrium mixture of two forms(called tautomers) -when iron(III) chloride is added to ethylaccetoacetate the solution becomes coloured because of a reaction between the enol form and the iron(III) chloride. The enol form of ethylacetoacetate also reacts with bromine water.

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