The catalytic destruction of ozone occurs via a two-stepmechanism, where X can be any of several species:(1)X+O₃→XO+O₂ [slow](2) XO+O→XO₂ [fast](a) Write the overall reaction.(b) Write the rate law for each step.(c) X acts as ______, and XO acts as ______.(d) High-flying aircraft release NO into the stratosphere, which catalyzes this process. When O₃ and NO concentrations are 5X10¹² molecule/cm³ and 1.0X10⁹ molecule/cm³, respec-tively, what is the rate of O₃ depletion (k for the rate-determining step is 6X10⁻¹⁵cm³/molecule s)?
The catalytic destruction of ozone occurs via a two-stepmechanism, where X can be any of several species:(1)X+O₃→XO+O₂ [slow](2) XO+O→XO₂ [fast](a) Write the overall reaction.(b) Write the rate law for each step.(c) X acts as ______, and XO acts as ______.(d) High-flying aircraft release NO into the stratosphere, which catalyzes this process. When O₃ and NO concentrations are 5X10¹² molecule/cm³ and 1.0X10⁹ molecule/cm³, respec-tively, what is the rate of O₃ depletion (k for the rate-determining step is 6X10⁻¹⁵cm³/molecule s)?
For any chemical reaction rate law is defined as the change in any one of the reactants or products per unit time. Initially, there is no product, only reactant is present. As the reaction proceeds, Concentration of reactant decreases and concentration of product increases. So, the rate of the reaction can be described as :
Rate of the reaction= Decrease in the concentration of reactant/Time taken
Rate of the reaction =- []/
Rate of the reaction in terms of product= [P]/
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