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Calculate the pressure exerted by 5 mole of CO_(2) in one litre vessel at 47^@)C using van der Waal's equation. Also report the pressure of gas if it behaves ideal in nature. Given that a =3.592" atm It"^(2)" mol"^(-2), b=0.0427 It/mol. Also if the volume occupled by CO_(2) molecules is negligible, then calculate the pressure exerted by one mole of CO_(2) gas at 273 K. |
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Answer» Solution :van DER Waals equation `[P+(n^(2)a)/(V^(2))][V-nb]=NRT` `n_(CO_(2))=5, V=1" litre, "T=320 K, a=3.592, b=0.0427` `therefore [P+25xx(3.592)/(1)][1-5xx0.0427]=5xx0.0821xx320` `therefore P=77.218` atm For ideal behaviour of gas, PV =nRT `therefore P xx1=5xx0.0821xx320` `therefore P=131.36` atm For one mole `[P+(a)/(V^(2))][V-b]=RT` `therefore P =(RT)/(V) -(a)/(V^(2))` `therefore P =(0.0821xx273)/(22.4)-(3.592)/((22.4)^(2))` `therefore P =0.9922` atm The volume occupied by 1 mole at 273 K is 22.4 litre if b is negligible. |
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