Question

A sample of 16g charcoal was brought into contact with $C{H}_4$ gas contained in a vessel of 1 litre at $27^{0}C$ . The pressure of gas was found to fall from 760 to 608 torr. The density of charcoal sample is 1.6g/ $c{m}^3$. What is the volume of the $C{H}_4$ gas adsorbed per gram of the adsorbent at 608 torr and $27^{0}C$ ?

• A. 125 mL/g
• B. 16.25 mL/g
• C. 26 mL/g
• D. None of these

Answer 1

The correct option is B 16.25 mL/g

Final volume of gas, at $608$ torr pressure
$V_2=\frac{P_1{V}_1}{P_2}$
$=\frac{760\times 1}{608}$
$\Rightarrow$ $1.25$ or $V_2=1250mL$
Volume occupied by gas = Volume of vessel - Volume occupied by charcoal
$=1000-\frac{16}{1.6}=990mL$
Difference of volume is due to adsorption of gas by charcoal.
$\therefore$ Volume of gas adsorbed by charcoal
$=1250-990$
$\Rightarrow 260mL$
Volume of the gas adsorbed per gram of charcoal
$=\frac{260}{16}=16.25mL/g$ at $608$ torr and ${27}^{\circ }C$.