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A reaction is found to have the rate law:
$Rate = k [A]^{2} [B]$
Which set of data is consistent with this finding?
[A], mol $L^{- 1}$ [B], mol $L^{- 1}$ Rate mol $L^{- 1}$ $s^{- 1}$
Given 0.010 0.010 $1.2 \times 10^{- 4}$
A 0.010 0.020 $2.4 \times 10^{- 4}$
B 0.020 0.010 $6.0 \times 10^{- 4}$
C 0.020 0.020 $4.8 \times 10^{- 4}$
d 0.010 0.020 $4.8 \times 10^{- 4}$

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answer is A.

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Detailed Solution

$K = \frac{(1.2 \times 10^{- 4})}{{(0.010)}^{2} (0.010)} K_{A} = \frac{(2.4 \times 10^{- 4})}{{(0.010)}^{2} (0.020)} K_{A} = \frac{2 \times (1.2 \times 10^{- 4})}{2 \times {(0.010)}^{2} (0.010)} K_{A} = K$

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