Molecular weight of

aniline $=M.wt.$ of  $C _6 NH _7$

$=72+7+14=93$

$\text { density of } P=1 gm ml ^{-1}$

$9.3 ml \text { of } P=9.3 gm P$

$=\frac{9.3}{9.3}=0.1 mole P$

The mole ratio $PhNH _2: PhN _2{ }^{+}$:

(image)

$=1: 1: 1$

$\text { so the mole of } Q \text { formed will be } 0.1 \text { mole and extent of reaction is } 100 \% $$\text { but if it is } 75 \% \text { yield. }$

$\text { Then amount of } Q =0.1 \times \frac{75}{100}=0.075 mol$

$\text { The molecular formula of } Q = C _{16} H _{12} ON _2$

$\text { so M.wt. of } Q=16 \times 12+12 \times 1+16+2 \times 14$

$=192+12+16+28$

$=248 gm$

$\text { so amount of } Q =248 \times 0.075$

$=18.6 gm$