[" For reaction "NO_(2)+CO rarr CO_(2)+NO" ,the rate "],[" expression is,Rate "=K[NO_(1)]^(2)],[" The number of molecules of CO involved in the "],[" slowest step will be - "]

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)+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)+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 a reaction NO_(g) +O_(2) (g) rarr 2NO_(2)(g) Rate =k[NO^(2)] [O_(2)] if the volume of the reaction vessel is doubled the rate of the reaction :

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?