Question

How many gram of ethanol is required in the reaction with $Na$ metal in order to give $560ml$ dihydrogen gas at STP?

• A. $11.5$
• B. $1.15$
• C. $4.6$
• D. $2.3$

Answer 1

The correct option is D $2.3$

Reaction of ethanol $\left(C_2{H}_{5}OH\right)$ with $Na$ (Sodium) metal is as follows :

$2C_2{H}_{5}OH+2Na⟶2C_2{H}_{5}ONa+H_2$

$⟹$ $22.4L$ of $H_2⟶1$ Mole of $H_2.$

$560ml$ of $H_2⟶\frac{1}{40}$ mole of $H_2.$

$⟹1$ mole of $H_2$ requires $2$ moles of $C_2{H}_{5}OH$

$\frac{1}{40}$ mole of $H_2$ requires $\frac{2}{40}$ moles of $C_2{H}_{5}OH$

$⟹\frac{2}{40}$ Moles of $C_2{H}_{5}OH=\frac{2}{40}\times \left\{2\right(12)+5(1)+1(16)+1(1\left)\right\}=2.3g$