6. Using Le Châtelier\'s principle, predict what will happen to the equilibrium
ID: 1026978 • Letter: 6
Question
6. Using Le Châtelier's principle, predict what will happen to the equilibrium under the follow- ing conditions: (Hint: The Fe3+ ion is yellow and the [FeSCN2+ complex is red.) (3 points) CONDITION DIRECTION OF SHIFT PREDICTED OBSERVATION More Fe3+ is added Fe3+ is removed SCN- is added Predict whether the reaction will have a positive or negative AH value. Explain your answer using molecular level evidence. (3 points) 7. Predict whether the reaction will have a positive or negative AS value. Explain your answer using molecular level evidence. (3 points) 8.Explanation / Answer
Fe3+ + SCN- <---------> [FeSCN]2+
6) For the above equilibrium reaction,
If more Fe3+ is added then the equilibrium will shift towards right and the predicted observation is the
formation of red complex.
If Fe3+ is removed then the equilibrium will shift towards left (as it wants to be replaced) and the predicted
observation is colorless.
If SCN- is added then the equilibrium will shift towards right direction and predicted observation is the formation
of red complex.
7) There are more reactants(2) than products (1) , hence Keq will decrease and H will be negative
(heat will be evolved).
8) Number of reactants > Number of products , i.e) the system is going from more randomness or disorder
to less disorder. Hence S will be negative.
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