Advertisements
Advertisements
Question
Can a Van der Waals gas with a = 0 be liquefied? explain.
Advertisements
Solution
- a = 0 for a Van der Waals gas i.e. for a real gas. Van der Waals constant a = 0. It cannot be liquefied.
- If a = 0, there is very less interaction between the molecules of gas.
- ‘a’ is the measure of the strength of Van der Waals force of attraction between the molecules of the gas.
- If a is equal to zero, the Van der Waals force of attraction is very less and the gas cannot be liquefied.
APPEARS IN
RELATED QUESTIONS
Maximum deviation from ideal gas is expected from
Which of the following diagrams correctly describes the behaviour of a fixed mass of an ideal gas? (T is measured in K)
25 g of each of the following gases are taken at 27°C and 600 mm Hg pressure. Which of these will have the least volume?
In what way real gases differ from ideal gases.
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if it is compressed to a smaller volume at a constant temperature.
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if the temperature is raised while keeping the volume constant.
Write the Van der Waals equation for a real gas. Explain the correction term for pressure and volume.
Value of universal gas constant (R) is same for all gases. What is its physical significance?
Pressure versus volume graph for a real gas and an ideal gas are shown in figure. Answer the following questions on the basis of this graph.
(i) Interpret the behaviour of real gas with respect to ideal gas at low pressure.
(ii) Interpret the behaviour of real gas with respect to ideal gas at high pressure.
(iii) Mark the pressure and volume by drawing a line at the point where real gas behaves as an ideal gas.
Assertion (A): At constant temperature, pV vs V plot for real gases is not a straight line.
Reason (R): At high pressure all gases have \[\ce{Z}\] > 1 but at intermediate pressure most gases have \[\ce{Z}\] < 1.
