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For the reaction:
$2 A + 3 B ⟶ C, [A]$ , is found to decrease at a rate of $2.0 M . s^{- 1}$ . If the rate law is rate= k[A], how fast does [B] decrease under the same conditions?

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2.0 $M . s^{- 1}$

0.66 $M . s^{- 1}$

1.3 $M . s^{- 1}$

3.0 $M . s^{- 1}$

answer is D.

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Detailed Solution

$\begin{array}{l} \frac{dx}{dt} = K [A] \\ - \frac{d [A]}{dt} = 2 .0 {MS}^{- 1} \end{array}$

$2 A + 3 B \to C$

$- \frac{1}{2} \frac{d [A]}{dt} = - \frac{1}{3} \frac{d [B]}{dt} = \frac{+ d [C]}{dt}$

$\frac{d [B]}{dt} = \frac{3}{2} \cdot \frac{d [A]}{dt} = - 3 .0 M . s^{- 1}$

$\frac{- d [B]}{dt} = 3 .0 {M . s}^{- 1}$

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