From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
`"(i)"3NO(g)toN_(2)O(g)Rate =K[NO]^(2)`
`"(ii)'H_(2)O_(2)(aq)+3I^(-)(aq)to 2H_(2)O(I)_(3)^(-) Rate=k[H_(2)O_(2)][I^(-)]`
`"(iii)" CH_(3)CHO(g)toCH_(4)(g)+CO(g)Rate =k[CH_(3)CHO]^(3//2)`
`"(iv)" C_(2)H_(5)Cl(g)to C_(2)H_(4)(g)+HCl(g) "Rate" = k[C_(2)H_(5)Cl]`

Answer

`a. OR=2`
`k=L mol^(-1)s^(-1)`
`b. OR(H_(2)O_(2))=1`
`OR(I^(c-))=1`
`OR(H^(o+))=0`
Overall`OR=2`
`k=L mol^(-1)s^(-1)`
`c. OR(CH_(3)CHO,Overall)=1.5`
`k=L^(1//2) mol^(-1//2 )s^(-1)`
`c. OR(CH_(2)H_(5)Cl)=1`
OR(Overall)=1
`k=s^(-1)`

Explanation

`a.` Order with respect to `NO` and overall order `=2`
`k=L mol^(-1)s^(-1)`
`b.` Order `w.r.t. H_(2)O_(2)=1`
Order `w.r.t. I^(c-)=1`
Order `w.r.t. H^(c-)=0`
Overall order order `=2`
`k=L mol^(-1)s^(-1)`
`c.` Order `w.r.t. CH_(3)CHO` and
Overall order `=1.5`
`k=L^(1//2) mol^(-1//2)s^(-1)`
`d.` Order `w.r.t. C_(2)H_(5)Cl=1`
Overall order `=1`
`k=s^(-1)`