The reaction between hydrochloric acid HCl and sodium thiosulfate Na2S2O3 can be represented by the following balanced chemical equation:2HCl aq + Na2S2O3 aq 2NaCl aq + H2O l + SO2 g + S s The effect of increasing pressure on the rate of this reaction can be analyzed using Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration of reactants or products, the system will adjust to counteract the change and re-establish equilibrium.In this reaction, there is a production of a gaseous product, sulfur dioxide SO2 . When the pressure is increased, the system will try to counteract the change by shifting the equilibrium position to the side with fewer moles of gas. In this case, the reaction will shift to the left toward the reactants because there are no gaseous reactants and only one gaseous product.However, it is important to note that the rate of the reaction is not solely determined by the pressure. Other factors, such as temperature and concentration of reactants, can also affect the reaction rate. In general, increasing the concentration of reactants or increasing the temperature will increase the rate of the reaction.In summary, increasing the pressure will shift the equilibrium position of the reaction between hydrochloric acid and sodium thiosulfate to favor the reactants, which may lead to a decrease in the rate of the reaction. However, the overall effect on the reaction rate will also depend on other factors, such as temperature and concentration of reactants.