Advertisements
Advertisements
Question
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.
Options
Both A and R are true and R is the correct explanation of A.
Both A and R are true but R is not the correct explanation of A.
A is true but R is false.
A is false but R is true.
Advertisements
Solution
Both A and R are true but R is not the correct explanation of A.
Explanation:
At constant temperature, the pV vs V plot for real gases is not a straight line because there is intermolecular attraction present in real gases which is absent in ideal gases; hence ideal gases form a straight line in the pV vs V plot at constant temperature.
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?
The value of the universal gas constant depends upon
Maximum deviation from ideal gas is expected from
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 the temperature is raised while keeping the volume constant.
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.
Which of the following gases would you expect to deviate from ideal behavior under conditions of low-temperature F2, Cl2, or Br2? Explain.
Under which of the following two conditions applied together, a gas deviates most from the ideal behaviour?
(i) Low pressure
(ii) High pressure
(iii) Low temperature
(iv) High temperature
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)`. 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.
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]
