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(g)+2H_(2)(g)toN_(2)(g)+2H_(2)O(g) . The rate law is rate =k[NO]^(2)[H_(2)] . What is the overall order of reaction.

For the reaction 2NO(g)+O_(2)(g)rarr2NO_(2)(g) , the rate law is r=k[NO]^(2)[O_(2)] . The reaction is carried out in a V L closed container . If the container had a volume equal to one-fourth of V L , then what would the reaction - rate be ?

For the reaction, 2NO_((g) + O_(2(g) rarr 2NO_(2(g) the rate law is given as. Rate =k [NO]^2[O_2] The order of the reaction with respect to O_2 is _______

For the reaction (Cl)_(2)(g)+2 (NO)(g) rarr 2 (NOCl)(g) the rate law is expressed as rate =(k)[(Cl)_(2)][(NO)]^(2) What is the overall order of this reaction.

In the reaction, 2NO(g)+O_(2)(g)rarr2NO_(2)(g) , the rate to change of concentration of NO is

For a reaction, Cl_(2)(g) + 2NO(g) to 2NOCl(g) ,the rate law is expressed as rate = k[Cl_(2)][NO]^(2) . What is the order of the reaction?

For the reaction : Cl_2 (g) + 2NO (g) rarr 2 NOCl(g) The rate law is expressed as rate = k[NO]^2 [Cl_2] What is the overall order of the reaction ?