Changing the pressure typically affects the rate of reaction for gaseous reactants and products. However, in the reaction between hydrochloric acid HCl and calcium carbonate CaCO3 , both reactants are in the solid or liquid phase, and the products are also in the solid or liquid phase, with the exception of carbon dioxide CO2 which is a gas.The reaction can be represented by the following balanced equation:2HCl aq + CaCO3 s CaCl2 aq + H2O l + CO2 g In this reaction, increasing the pressure would have a minimal effect on the rate of reaction. This is because the reaction rate is primarily influenced by the concentration of the reactants, temperature, and the presence of a catalyst, rather than the pressure.However, if the reaction is carried out in a closed system where the pressure can build up, the increased pressure may have a slight effect on the rate of reaction due to the production of CO2 gas. As the pressure increases, the equilibrium of the reaction may shift slightly, affecting the rate of reaction. But overall, the effect of pressure on this reaction is minimal compared to other factors such as concentration and temperature.