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The following results are obtained during the kinetic studies of the reaction. $2 A + B \overset{}{\to} C + D$
$[A]$ $[B]$ rate
I 0.1 m 0.1 m $6 \times 10^{- 3} M \min^{- 1}$
II 0.3 m 0.2 m $7.2 \times 10^{- 2} M \min^{- 1}$
III 0.3 m 0.4 m $28.8 \times 10^{- 2} M \min^{- 1}$
IV 0.4 m 0.1 m $2.40 \times 10^{- 2} M \min^{- 1}$
Rate law is given by

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$r = K {[A]}^{1} {[B]}^{1}$

$r = K {[A]}^{1} {[B]}^{2}$

$r = K {[A]}^{0} {[B]}^{2}$

$r = K {[A]}^{1} {[B]}^{0}$

answer is B.

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Detailed Solution

On doubling the concentration of B keeping A constant rate becomes four times. order w.r.to B is 2
If concentration of $[A]$ is increased by 4 times keeping (B) constant rate increases by 4 times.
order with respect to $[A]$ is 1

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