Advertisements
Advertisements
Question
In what way real gases differ from ideal gases.
Advertisements
Solution
- Ideal gases are the gases that obey gas laws or gas equation PV = nRT.
- Real gases do not obey gas equation. PV = nRT.
- The deviation of real gases from ideal behaviour is measure in terms of a ratio of PV to nRT. This is termed as compression factor (Z). Z = `"PV"/"nRT"`
- For ideal gases Z = 1.
- For real gases Z > 1 or Z < 1. For example, at high-pressure real gases have Z >1 and at intermediate pressure Z < 1.
- Above the Boyle point Z > 1 for real gases and below the Boyle point, the real gases first show a decrease for Z, reach a minimum and then increase with the increase in pressure.
- So, it is clear that at low pressure and high temperature, the real gases behave as ideal gases.
APPEARS IN
RELATED QUESTIONS
Calculate the volume occupied by 8.8 g of CO2 at 31.1°C and 1 bar pressure. R = 0.083 bar L K–1 mol–1.
Which of the following is the correct expression for the equation of state of van der Waals gas?
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)
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if it is compressed to a smaller volume at a constant temperature.
Which of the following gases would you expect to deviate from ideal behavior under conditions of low-temperature F2, Cl2, or Br2? Explain.
If 1 gram of each of the following gases are taken at STP, which of the gases will occupy (a) greatest volume and (b) smallest volume?
\[\ce{CO, H2O, CH4 , NO}\]
Value of universal gas constant (R) is same for all gases. What is its physical significance?
Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. What is the value of Z for an ideal gas?
In van der Waal's equation for the real gas, the expression for the net force of attraction amongst the gas molecules is given by:
