The reaction, `2NO+Br_(2)rarr 2NOBr`, is supposed to follow the following mechanism, (i) `NO+Br_(2) overset("fast")(hArr) NOBr_(2)` (ii) `NOBr_(2) +NO
The reaction, `2NO+Br_(2)rarr 2NOBr`, is supposed to follow the following mechanism,
(i) `NO+Br_(2) overset("fast")(hArr) NOBr_(2)`
(ii) `NOBr_(2) +NO overset(slow)(rarr)2NOBr`
suggest the rate law expression.
A. `r=k[NO]^(2)[Br_(2)]`
B. `r=k[NO][Br_(2)]`
C. `r=k[NO][Br_(2)]^(2)`
D. `r=k[NOBr_(2)]`
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Correct Answer - A
(a) For slowet step : rate
`=k[NO][Br_(2)]" "...(i)`For equilibrium,
`k=([NOBr_(2)])/([NO][Br_(2)])" "...(ii)`by(i) and(ii),
`r=k dot"K_(c)[NO]^(2) [Br_(2)]`
rate
`=k[NO]^(2)[Br_(2)]`
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