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For the reaction 2A + B → C + D, measurement of rule of reaction at varying concentrations are given below
Exp. no. (A) (B) Rate (m mole lit-1 sec-1)
1 0.010 0.010 2.5
2 0.010 0.020 5.0
3 0.030 0.020 45.0
The rate law is therefore

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$Rate =$ $k {[A]}^{2} [B]$

$Rate = k [A] {[B]}^{2}$

$Rate = k [A] [B]$

$Rate = k {[A]}^{2} {[B]}^{2}$

answer is A.

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Detailed Solution

$Rate = k {(A)}^{m} {(B)}^{n} 2.5 = k {(0.01)}^{m} {(0.01)}^{n} - - - - - - - 1 5.0 = k {(0.01)}^{m} {(0.02)}^{n} - - - - - - - 2 45 = k {(0.03)}^{m} {(0.02)}^{n} - - - - - - - - 3 On solving, m = 2, n = 1$

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