A chemical system at equilibrium is disturbed such that it undergoes a change in concentration. Which statement about this system is true?
a) An increase in product concentration will result in a shift to product formation.
b) A decrease in product concentration will result in a shift to reactant formation.
c) An increase in product concentration will not affect product formation.
d) A decrease in product concentration will not affect reactant formation.
e) An increase in product concentration will not affect Keq.
b) A decrease in product concentration will result in a shift to reactant formation.
are you sure?
Yes, I apologize for the incorrect response. The correct statement is:
a) An increase in product concentration will result in a shift to reactant formation.
What is the correct answer?
Apologies for the confusion. The correct answer is:
c) An increase in product concentration will not affect product formation.
To determine the true statement about the chemical system at equilibrium when the concentration is changed, we need to understand Le Chatelier's principle.
Le Chatelier's principle states that when a system at equilibrium is disturbed, it will shift in a way that counteracts the disturbance. The system will try to reach a new equilibrium by adjusting the ratio of reactants and products.
In the given question, if the concentration of a product in the chemical system at equilibrium is increased, the system will try to counteract this disturbance. This means the system will shift towards the reactant formation to consume the excess product and try to establish a new equilibrium.
So, the true statement about the system is:
b) A decrease in product concentration will result in a shift to reactant formation.