Advertisements
Advertisements
प्रश्न
In what way real gases differ from ideal gases.
उत्तर
- 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
संबंधित प्रश्न
Which of the following is the correct expression for the equation of state of van der Waals gas?
The value of the universal gas constant depends upon
Maximum deviation from ideal gas is expected from
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?
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if it is compressed to a smaller volume at a constant temperature.
Write the Van der Waals equation for a real gas. Explain the correction term for pressure and volume.
Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. What is the value of Z for an ideal gas?
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.
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:
Choose the correct option for the total pressure (in atm.) in a mixture of 4g \[\ce{O2}\] and 2g \[\ce{H2}\] confined in a total volume of one litre at 0°C is ______.
[Given R = 0.082 L atm mol−1K−1, T = 273 K]
