1.

A reaction is first order in A and second order in B. (i) Write differential rate equation. (ii) How is rate affected when concentrated of B is tripled ? (iii) How is rate affected when concentration of both A and B is doubled ?

Answer»

Solution :(a) A + B = Products.
(i) The reaction is of Ist order with respect to A.
Rate w.r.t. `[A] = k[A]`
it is of SECOND order w.r.t. B.
Rate w.r.t. `[B] = k[B]^(2)`
`:.` Overall rate of reaction `= k[A][B]^(2)`
`:. (DX)/(dt) = k[A][B]^(2)`
(ii) When the concentration of B is tripled.
`r^(2) = k[A][3B]^(2)`.
`=9K[A][B]^(2)`
`:.` Rate becomes 9 times.
(iii) If the concentration of A and B is doubled, then
`r = k[2A][2B]^(2)`
`= 8k[A][B]^(2)`
`:.` Rate becomes 8 times.


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