Problem 60
According to kinetic theory of gases, the collisions between molecules of a gas (a) occur in a zig-zag path (b) occur in a straight line (c) change velocity and energy (d) result in settling down of molecules.
Problem 61
Which of the following assumptions is incorrect according to kinetic theory of gases? (a) Particles of a gas move in all possible directions in straight lines. (b) All the particles, at any particular time, have same speed and same kinetic energy. (c) There is no force of attraction between the particles of a gas at ordinary temperature and pressure. (d) The actual volume of the gas is negligible in comparison to the empty space between them.
Problem 62
A gas that follows Boyle's law, Charles' law and Avogadro's law is called an ideal gas. Under what conditions a real gas behaves as ideal gas? (a) Under low pressure and temperature (b) Under high pressure and temperature (c) Under high pressure and low temperature (d) Under low pressure and high temperature
Problem 63
If the assumption that there is no force of attraction between the molecules of a gas is correct, what will be the consequences? (a) All gases will be ideal gases. (b) The gases will never liquefy when cooled and compressed. (c) Gases will have definite volume. (d) Gases will occupy a definite space.
Problem 65
A gas deviates from ideal behaviour at a high pressure because its molecules (a) have kinetic energy (b) are bound by covalent bonds (c) attract one another (d) show the Tyndall effect.
Problem 67
Taking into account the pressure and volume corrections, the gas equation can be written as (a) \(\left(P+\frac{a^{2}}{V^{2}}\right)(V-b)=n R T\) (b) \(\left(P+\frac{a n^{2}}{V^{2}}\right)(V-n b)=n R T\) (c) \(\left(P+\frac{a V}{n R T}\right)\left(\frac{V-b}{n R T}\right)=R T\) (d) \(\left(P+\frac{Z}{V^{2}}\right)(V-Z b)=n R T\)
Problem 69
The unit of \(a\) in van der Waals equation, \(\left(P+\frac{a n^{2}}{V^{2}}\right)(V-n b)=n R T .\) is (a) \(\mathrm{atm} \mathrm{L}^{2} \mathrm{~mol}^{-2}\) (b) atm \(\mathrm{L} \mathrm{mol}^{-2}\) (c) \(\operatorname{atm} \mathrm{L} \mathrm{mol}^{-1}\) (d) \(\mathrm{atm} \mathrm{L}^{2} \mathrm{~mol}^{-1}\)
Problem 70
In van der Waals equation for a non-ideal gas, the term that accounts for intermolecular force is (a) \((V-b)\) (b) \(\left(P+\frac{a}{V_{-}^{2}}\right)\) (c) \(R T\) (d) \(P V\)
Problem 73
In the corrections made to ideal gas equation for real gases, the reductions in pressure due to forces of attractions between the molecules is directly peoportional to (a) \(\frac{n}{V}\) (b) \(\frac{n^{2}}{V^{2}}\) (c) \(\boldsymbol{V}-\boldsymbol{n} b\) (d) \(n b\)
Problem 74
A real gas obeying van der Waals equation will resemble ideal gas, if the (a) constents a and \(b\) both are small (b) \(\boldsymbol{a}\) is arge and \(b\) is small (c) \(a\) is \(\mathrm{small}\) and \(b\) is large (d) constants \(a\) and \(b\) both are large.
