Find overall order of given reaction using following experimental data
`2NO+Cl_2to2NOCl`

Find overall order of reaction if rate law expression are as follows:- (a) rate =K[CO]^(2)[Cl_(2)]^(0.5) (ii) rate =K[CH_(3)COOC_(2)H_(5)]^(1)[H_(2)O]^(0)

The form of rate law for a reaction is expressed as, rate = k [Cl_(2)][NO]^(2) Find out the order of the reaction with respect to Cl_(2) , with respect to NO and also the overall order of the reaction.

Define the order of chemical reaction . Find the overall order of the following reactions : (a) CHCl_(3(g)) +Cl_(2(g))rarr C Cl_(4(g))+HCl_((g)),"Rate"= k[CHCl_(3)][Cl_(2)] (b) 2NO_((g))+O_(2(g)) rarr 2NO_(2(g)),"Rate" = k[NO]^(2)[O_(2)]

For a reaction 2P + Q to S , following data were collected. Calculate the overall order of the reaction. Also find out the reaction rate constant.

The reaction between NO and Cl_(2) takes place in the following two steps : I {:(" "k_(1)), (NO + Cl_(2) hArr NOCl_(2)), (" "k_(2)), (" ""fast"):} II. NOCl_(2)underset("fast")overset(k_(2))rarr2NOCl The rate law of overall reaction, 2NO+Cl_(2)to2NOCl can be given by:

2 NO(g)+Cl_2(g) = 2NOCl(s) This reaction was studied at -10^@C and the following data was obtained {:(run,[NO]_0,[Cl_2]_0,r_0),(1,0.10,0.10,0.18),(2,0.10,0.20,0.35),(3,0.20,0.20,1.40):} [NO]_0 and [Cl_2]_0 are the initial concentrations and r_0 is the initial reaction rate The overall order of the reaction is ___________ . (Round off to the Nearest Integer).

For the reaction , H_(2)(g) + Cl_(2) (g) to 2HCI(g) The experimental data suggests r = k[H_(2)] [Cl_(2)]^((1)/(2)) The molecularity and order for the reaction is