Consider the following equilibrium reaction having gaseous reactants and products.
4HCl + O2 ⇌ 2H2O + Cl2
Which of the following would result from increasing the concentration of H2O?
The rate of the backward reaction increases.
The concentration of hydrochloric acid decreases.
The rate of forward reaction increases.
The concentration of chlorine increases.
Answers
Answer:
Consider the following equilibrium reaction having gaseous reactants and products. 4HCl + O2 ⇌ 2H2O + Cl2 Which of the following would result from increasing the concentration of H2O? The rate of the backward reaction increases.
Answer:
On increasing the concentration of H₂O, the rate of backward reaction increases.
Explanation:
Le-Chatlier's principle states that on changing any of the factors that determine the equilibrium conditions of a system, the system will move in such a direction so that the change is balanced.
According to Le-Chatlier's principle, the change in concentration caused by adding a reactant/product is relieved by shifting the net reaction in that direction where the added substance gets consumed. In other words, if the reactant concentration increases or the product concentration decreases, the equilibrium will shift in the forward direction. On the other hand, if the product concentration increases or the reactant concentration decreases, the equilibrium will shift in the backward direction.
Here on increasing the concentration of H₂O(concentration of product increases), the equilibrium will shift in the backward direction or the rate of backward reaction increases.