For a hypothetical reaction
$A + 3 B ⟶ P Δ H = - 2 x kJ / mole$ of A and $M ⟶ 2 Q + R Δ H = + x kJ / mole$ of M If these reactions are carried simultaneously in a reactor such that temperature is not changing. If rate of disappearance of B is y ${M sec}^{- 1}$ then rate of formation $(in M \sec^{- 1})$ of Q is :

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$\frac{4}{3} y$

$\frac{2}{3} y$

$\frac{3}{4} y$

$\frac{3}{2} y$

answer is C.

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Detailed Solution

$\begin{array}{l} - \frac{1}{3} \frac{d [B]}{d t} = - \frac{d [A]}{d t} \\ - \frac{d [M]}{d t} = \frac{1}{2} \frac{d [Q]}{d t} \\ (\frac{- d [A]}{d t}) \times 2 = \frac{- d [M]}{d t} \\ \frac{2 y}{3} = \frac{1}{2} \frac{d [Q]}{d t} \end{array}$

or $\frac{d [Q]}{d t} = \frac{4 y}{3}$

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