Consider the following statements. (I) A gas above its critical temperature cannot be liquefied by the application of pressure. (II) At the Boyle temperature, Z of a real gas stays close to 1 over a w

Question

Consider the following statements.

(I) A gas above its critical temperature cannot be liquefied by the application of pressure.

(II) At the Boyle temperature, Z of a real gas stays close to 1 over a wide range of low pressures.

(III) For a van der Waals gas, the critical temperature is greater than the Boyle temperature.

Which of the statements are correct?

TestHub · Accepted Answer

(I) True: no pressure can liquefy a gas above $T_{c}$ .

(II) True: at $T_{B}$ the slope $d Z / d P$ is zero at low pressure.

(III) False: $T_{c} = (8/27) T_{B}$ , so $T_{c}$ is less than $T_{B}$ .

Answer: (B).

Chemistry - Real Gas Question with Solution | TestHub