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A reaction is first order in A and secon...

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 ?

Text Solution

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(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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Knowledge Check

  • For a chemical reaction A+B rarr C it has been found that : (i) rate becomes double when the concentrations of A is doubled (ii) rate becomes 16 times when the concentrations of both A and B are doubled . The rate expression is :

    A
    rate `= k[A]^(2) [B]`
    B
    rate `= k[A][B]^(2)`
    C
    rate = `k[A][B]^(3)`
    D
    rate `= k[A]^(2)` .

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