According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust itself to counteract that change and restore the equilibrium. In this case, the reaction can be represented as:2NO g 2NO g + O g If the concentration of nitrogen dioxide NO is increased in the container, the system will try to counteract this change by shifting the equilibrium position to consume the excess NO. This means that the reaction will shift to the right, producing more nitrogen oxide NO and oxygen gas O until a new equilibrium is established.To restore the original equilibrium position, the student can either:1. Remove some of the excess NO from the container, which will cause the system to shift back to the left, decreasing the concentrations of NO and O and increasing the concentration of NO until the original equilibrium position is reached.2. Increase the volume of the container, which will decrease the overall pressure of the system. According to Le Chatelier's principle, the system will respond by shifting the equilibrium position to the side with more gas molecules, in this case, the left side. This will result in an increase in the concentration of NO and a decrease in the concentrations of NO and O until the original equilibrium position is reached.3. Decrease the temperature of the system, assuming the reaction is exothermic. Lowering the temperature will cause the system to shift in the direction that releases heat, which is the reverse reaction left side . This will increase the concentration of NO and decrease the concentrations of NO and O until the original equilibrium position is reached.