For the reaction between nitrogen monoxide+ oxygen= nitrogen dioxide , If volume of the product nitrogen dioxide is being increased, where will equilibrium shift to and why will it have to shift that way?
According to Le Chatelier's Principle, if the volume of the product nitrogen dioxide is increased, the equilibrium will shift to the right in order to minimize the stress caused by the increase in volume. By shifting to the right, more nitrogen monoxide and oxygen will react to form nitrogen dioxide, therefore increasing the amount of nitrogen dioxide and thereby decreasing the volume of gases present in the system. This allows the system to relieve the stress caused by the increase in volume and reach a new equilibrium position.
