For the reaction `NO_(2)+COrarrCO_(2)+NO`, the experimental rate expresison is `-dc//dt = k[NO_(2)]^(2)`. Find the number of molecules of `CO` involved in the slowest step.

For the reaction NO_(2)(g) + CO(g) to NO(g) + CO_(2)(g) , the experimentally determined rate expression at 40 K is: rate = k[NO_(2)]^(2) What is the proposed mechanism for the reaction?

For the reaction NO_(2)+CO to CO_(2)+NO , the rate law is : Rate =k[NO_(2)]^(2) . Propose the probable mechanism of this reaction.

For the reaction : 2NO_(2)(g)+F_(2)(g)rarr2NO_(2)F(g) the rate law is , rate =k[NO_(2)][F_(2)] . Write the differential rate equation for the reaction.

For the reaction 2NO_(2)rarrN_(2)O_(3)+O_(2) , rate expression is as follows : -(d[NO_(2)])/(dt)=K[NO_(2)]^(n) , where K=3xx10^(-3)mol^(-1)L sec^(-1) If rate of formation of oxygen is 1.5xx10^(-4)mol L^(-1)sec^(-1) then the molar concentration of NO_(2) in mole L^(-1) is :