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9 February, 21:03

Consider the following system at equilibrium:

D (aq) + E (aq) F (aq)

Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.

Increase D

Increase E

Increase F

Decrease D

Decrease E

Decrease F

Triple D and reduce E to one third

Triple both E and F

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  1. 9 February, 21:21
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    Increase D ⇒ rightward shift

    Increase E ⇒ rightward shift

    Increase F ⇒ leftward shift

    Decrease D ⇒ leftward shift

    Decrease E ⇒ leftward shift

    Decrease F ⇒ rightward shift

    Triple D and reduce E to one third ⇒ no shift

    Triple both E and F ⇒ no shift

    Explanation:

    Changes in the concentrations of reactants y products affect to the equilibrium. In this case, D and E are reactants and F is the product.

    When a change in the factors affecting equilibrium occur, the system will react in order to counteract the change imposed.

    If a increase of reactant occur, the system will tend to produce more products (rightward shift). For example: increase D, increase E. In contraposition, if a decrease of reactant occur, the system will produce more reactants (leftward shift). For example: decrease D, decrease E. If a increase of product occur, the system will tend to produce more reactants (leftward shift). For example: increase F. In contraposition, if a decrease of product occur, the system will produce more products (rightward shift). For example: decrease F. If we change both reactants and products concentration in the same amount, the net change is zero, so there is not shift. For example: Triple D and reduce E to one third (D x 3 and E/3, there is not change in the total amount of reactants); Triple both E and F (E x 3 and F x 3, the net change is zero).
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