The following mechanism has been proposed for the reaction of nitric oxide and chlorine: 1. NO(g) + Cl 2 (g) ---> NO

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The following mechanism has been proposed for the reaction of
nitric oxide and chlorine:

1. NO(g) +
Cl 2 (g)
--->
NOCl 2 (g) ;

(slow)
2.
NOCl 2 (g) +
NO(g) ---> 2 NOCl(g) ;
(fast)

a) Each of the reactions in the mechanism is called
a(n) reaction.

b) Select the correct number from below for the overall
reaction.
I. 2
NO( g ) +
NOCl 2 ( g ) --->
NOCl( g ) + 2 NO( g ) +
Cl( g )
II. NOCl 2 ( g )
+ Cl 2 (g) --->
NOCl( g ) + 3Cl( g )
III. 2
NO( g ) +
Cl 2 ( g ) ---> 2
NOCl( g )
IV. NO( g )
+ NOCl( g ) +
Cl 2 ( g ) --->
NOCl 2 ( g ) +
NOCl( g )
c) Identify all intermediates, if any:
(Write formulas without subscripts using the symbol “&”
without spacing between formulas if there is more than one.
Example, if Cl 2 write as
“Cl2”; if Cl 2 and NOCl
write as “Cl2&NOCl”; if
Cl 2 ,
NOCl 2 and NO write as
“Cl2&NOCl2&NO”, and so on.)

d) What is the molecularity (unimolecular, bimolecular,
etc. ) of step 2?

e) Write the overall rate law for this reaction? R
= k
(Write the rate law without any
spacing between the terms, without using subscripts
in the chemical formulas and with { } for the
molar concentration. For example, the rate law R
= k {H2 }3 {NO}1 would
be written “ R
= k {H2}3{NO}1 ” etc. The
first 3 characters-- R, =, and k -- are given in
the rate laws below. Complete the rest of the rate equations.)