The reaction between nitrogen gas N and oxygen gas O to form nitrogen dioxide gas NO can be represented by the following balanced chemical equation:N g + 2 O g 2 NO g The equilibrium constant, Kc, for this reaction can be expressed as:Kc = [NO] / [N] [O] where [NO], [N], and [O] represent the equilibrium concentrations of NO, N, and O, respectively.The relationship between the concentration of reactants and products and the equilibrium constant for this reaction can be understood using Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust its position to counteract the change and restore equilibrium.In the context of this reaction, if the concentration of reactants N and O is increased, the system will shift towards the products NO to restore equilibrium. This will result in an increase in the concentration of NO. Conversely, if the concentration of products NO is increased, the system will shift towards the reactants N and O to restore equilibrium, resulting in a decrease in the concentration of NO.However, it is important to note that the equilibrium constant, Kc, remains constant at a given temperature, regardless of the initial concentrations of reactants and products. This is because Kc is only dependent on temperature and not on the concentrations of reactants and products. Therefore, while the concentrations of reactants and products may change to restore equilibrium, the value of Kc will remain the same.In summary, the relationship between the concentration of reactants and products and the equilibrium constant for this reaction can be explained by Le Chatelier's principle. The system will adjust its position to counteract changes in the concentrations of reactants and products to restore equilibrium, but the value of Kc will remain constant at a given temperature.