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 DIncrease EIncrease FDecrease DDecrease EDecrease FTriple D and reduce E to one thirdTriple both E and F

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

This question is based on Le Chatelier's principle.

Le Chatelier's principle is an observation about chemical equilibria of reactions. It states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.

Increase D

D is a reactant. if we add reactants to the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Increase E

E is a reactant. if we add reactants to the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Increase F

F is a product. If we add additional product to a system, the equilibrium will shift to the left, in order to produce more reactants. The reaction would shift to the left.

Decrease D

if we remove reactants from the system, equilibrium will be shifted to the left.

Decrease E

if we remove reactants from the system, equilibrium will be shifted to the left.

Decrease F

if we remove products from the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Triple D and reduce E to one third

no shift in the direction of the net reaction, Both changes cancels each other.

Triple both E and F

no shift in the direction of the net reaction, Both changes cancels each other.