Question

Consider the following system at equilibrium:

Answer 1

Answer:

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).