Advertisements
Advertisements
प्रश्न
Value of universal gas constant (R) is same for all gases. What is its physical significance?
Advertisements
उत्तर
Unit of R depends on the units of p, V and T are measured, We know, `R = (pV)/(nT)`
Now, let's say, the pressure is measured in Pascal, per mole volume is measured in m3 and temperature is measured in Kelvin, then. Units of ‘R’ are Pa m3K–1 mol–1. Also, R is work done per mole per kelvin. It’s unit is J K–1 mol–1 (Joule is the unit of work done).
APPEARS IN
संबंधित प्रश्न
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?
The value of the universal gas constant depends upon
Compressibility factor for CO2 at 400 K and 71.0 bar is 0.8697. The molar volume of CO2 under these conditions is
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?
Can a Van der Waals gas with a = 0 be liquefied? explain.
Suppose there is a tiny sticky area on the wall of a container of gas. Molecules hitting this area stick there permanently. Is the pressure greater or less than on the ordinary area of walls?
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 more gas is introduced into the same volume and at the same 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?
Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. For real gas what will be the effect on value of Z above Boyle’s temperature?
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.
Isotherms of carbon dioxide gas are shown in figure. Mark a path for changing gas into liquid such that only one phase (i.e., either a gas or a liquid) exists at any time during the change. Explain how the temperature, volume and pressure should be changed to carry out the change.
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]
