The decomposition of hydrogen peroxide H2O2 is a first-order reaction, which means that the reaction rate depends only on the concentration of hydrogen peroxide itself and not on the concentration of any other reactants or products. The reaction can be represented by the following equation:2 H2O2 aq 2 H2O l + O2 g In general, the rate of a reaction can be affected by factors such as temperature, pressure, and the presence of catalysts. However, since the decomposition of hydrogen peroxide is a first-order reaction, changes in pressure will not have a significant effect on the reaction rate.This is because the rate law for a first-order reaction is given by:Rate = k[H2O2]where Rate is the reaction rate, k is the rate constant, and [H2O2] is the concentration of hydrogen peroxide. As you can see, the reaction rate depends only on the concentration of hydrogen peroxide and the rate constant, which is a temperature-dependent factor.However, it is important to note that if the reaction is carried out in a closed system, an increase in pressure could lead to an increase in the concentration of hydrogen peroxide, which in turn could result in a faster reaction rate. But this effect would be indirect and not a direct consequence of the pressure change itself.In summary, the reaction rate of the decomposition of hydrogen peroxide is not directly affected by changes in pressure. However, if the pressure change leads to a change in the concentration of hydrogen peroxide in a closed system, then the reaction rate could be indirectly affected.