Q. 33

# The critical temperature (T _{c}) and critical pressure (P_{c}) of CO_{2} are 30.98°C and 73atm respectively. Can CO_{2}(g) be liquefied at 32°C and 80atm pressure?

Answer :

The critical temperature (T_{c}) of any gasis defined as the value of temperature above which no gas can be liquefied, and the pressure at the critical temperature is calledcritical pressure (P_{c}).

So, as the CO_{2} gas cannot be liquefied at temperature which is greater than its critical temperature i.e 30.98°C even by applying any pressure. So as the given temperature is 32°C by applying a pressure of 80atm the CO_{2} gas cannot be liquefied.

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PREVIOUSCompressibility factor, Z, of a gas is given as Z = PV/ nRT(i) What is the value of Z for an ideal gas?(ii) For real gas what will be the effect on value of Z above Boyle’s temperature?NEXTFor real gases the relation between p, V and T is given by van der Waals equation:P + an2(V - nb) / V2= nRTWhere‘a’ and ‘b’ are van der Waals constants, ‘nb’ is approximately equal to the total volume of the molecules of a gas.‘a’ is the measure of magnitude of intermolecular attraction.(i) Arrange the following gases in the increasing order of ‘b’. Give reason. O2, CO2, H2, He(ii) Arrange the following gases in the decreasing order of magnitude of ‘a’. Give reason. CH4, O2, H2

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