" 24.For the reaction: "2NO+Br_(2)rarr2NOBr" ; Rate "=k[NO]^(2)[Br_(2)]." Write the proposed mechanism."

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 rection 2NOBr(g) rarr 2NO_2(g)+Br(g) , the rate law is rate = k[NOBr]^2 . If the rate of reaction is 6.5x10^(-6)mole L^(-1) s the concentration of NOBr is 2xx10^(-3) mole L^(-1) . What be the rate constant for the reaction?

In the reaction 2Br^(-) + X_(2) rarr Br_(2) + 2X^(-) , X_(2) is

The reaction rate of the reaction H_(2)(g)+Br_(2)(g)rarr2HBr(g) is given by r=k[H_(2)][Br_(2)]^(1//2) Which of the following statement/is/are true ?

2NOBr rarr 2NO(g)+Br_2(g) Rate= k[NOBr]_2 What are the units of rate constant.?

The reaction 2NO + Br_2rarr 2NOBr , obey.s the following mechanism:

For the reaction 2NOBr to 2NO_2 + Br_2, the rate law is rate = k[NOBr]^2 . If the rate of a reaction is 6.5xx10^(-6) molL^(-1)s^(-1) , when the concentration of NOBr is 2xx10^(-3) molL^(-1) .What would be the rate constant of the reaction?