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Question

A one litre vessel contained a gas at 270C. 6 g of charcoal was introduced into it. The pressure of gas fell down from 700 mm Hg to 400 mm Hg. Calculate the volume of the gas (at NTP) adsorbed per gram of charcoal. Density of charcoal sample used was 1.5 g cm−3.

A
60.107 cm3
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B
360.642 cm3
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C
120.214 cm3
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D
None of these
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Solution

The correct option is A 60.107 cm3
P1=700mm Hg=700/760 atm,V1=1L,T=27oC=300K,R=0.0821atmLmol1K1

Initial number of moles of gas (n1)=P1V1RT=(700/760)×10.0821×300 =0.0374 mol

volume occupied by charcoal =61.5=4 cm3

Available volume for the gas =(10004)=996 cm3

P2=700mm Hg=700/760 atm,V2=0.996L

Final number of moles (n2)=(400/760)×0.9960.0821×300=0.0213 mol

Number of moles of gas adsorbed =0.03740.0213=0.0161 mol

So, 6 gm of charcoal has adsorbed =0.0161 mol

Option A is correct.
1 gm of charcoal has adsorbed =0.01616 mol

Volume of gas adsorbed by 1 g charcoal at NTP.

=0.01616×22400=60.107 cm3

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