Question

Calculate the volume of hydrogen required for complete hydrogenation of $0.25d{m}^3$ of ethyne at STP.0.25dmof

• A. $0.25d{m}^3$
• B. $0.125d{m}^3$
• C. $0.5d{m}^3$
• D. none of these

Answer 1

The correct option is C $0.5d{m}^3$

Hydrogenation of ethyne in two process

$C_2{H}_2{+H}_2\to C_2{H}_4$

$C_2{H}_4+H_2\to C_2{H}_6$

By adding this,

$C_2{H}_2+{2H}_2\to C_2{H}_6$

Hence, for 1 mole hydrogenation of ethyne 2 mole of $H_2$ is required

So, 22.4L, hydrogenation\quad of\quad $C_2{H}_2$, $2\times 22.4l$ Of $H_2$ is required

So, 0.25L hydrogenation of $C_2{H}_2$, $2\times 0.25l$ of $H_2$ is required$

Hence 0.5 L or $0.5d{m}^3$ volume of $H_2$ is required.