In this PLE we are going to investigate Le Chatelier's Principle. This principle is stated, if a chemical reaction at equilibrium is subjected to a change in conditions that displaces it from equilibrium, then the reaction proceeds toward a new equilibrium state in the direction that offsets the change in conditions.

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Laboratory Section:

1. Consider the reaction,

2NO(g) + Br2(g) 2NOBr(g)

for which K = 160 at a particular temperature. A 1.0 liter container is found to contain 0.1 mol of NOBr, 0.0075 mol of NO and 0.9 mol of Br2. Is this reaction at equilibrium? Explain.

2. Consider the reaction,

2NO(g) + Br2(g) 2NOBr(g)

for which K = 160 at a particular temperature. The reaction is allowed to attain equilibrium. The concentration of each species at equilibrium in a 1.0 liter container was found to be, 0.075 M NOBr, 0.0019 M NO and 0.103 M Br2. If 0.01 mol of NOBr is added to this reaction in the 1.0 liter container, what is the new concentration of NOBr the instant the NOBr is added?

3. Is the system still at equilibrium? Explain. (Hint: what is Q under the new conditions?)

4. Which direction will the reaction proceed to re-establish equilibrium?

5. Consider a new 1.0 liter container with the reaction,

2NO(g) + Br2(g) 2NOBr(g)

at equilibrium. If some NOBr is removed, which direction will the reaction proceed to re-establish equilibrium? Explain.

6. Is there anything about the reaction or the questions that you feel you do not understand? List your concerns/questions.