The effect of increasing pressure on the rate of a chemical reaction that produces nitrogen dioxide gas depends on the specific reaction and the reaction conditions. In general, increasing the pressure will affect the reaction rate in one of the following ways:1. If the reaction involves a decrease in the number of moles of gas, increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas, according to Le Chatelier's principle. This will result in an increased rate of reaction, as the system tries to counteract the change in pressure.2. If the reaction involves an increase in the number of moles of gas, increasing the pressure will shift the equilibrium position towards the side with more moles of gas, according to Le Chatelier's principle. This will result in a decreased rate of reaction, as the system tries to counteract the change in pressure.3. If the reaction involves no change in the number of moles of gas, increasing the pressure will have no effect on the equilibrium position. However, increasing the pressure can still affect the rate of reaction by increasing the collision frequency between the reacting molecules. This can lead to an increased rate of reaction, as the probability of successful collisions between reactant molecules is higher.In summary, the effect of increasing pressure on the rate of a chemical reaction that produces nitrogen dioxide gas depends on the specific reaction and the reaction conditions. It can either increase or decrease the rate of reaction, depending on the change in the number of moles of gas involved in the reaction and the effect on collision frequency between reacting molecules.