If \(V_\text{H}\),\(V_\text{N}\) and \(V_\text{O}\) denote the root-mean square velocities of molecules of hydrogen, nitrogen and oxygen respectively at a given temperature, then:
1. \(V_\text{N}>V_\text{O}>V_\text{H}\)
2. \(V_\text{H}>V_\text{N}>V_\text{O}\)
3. \(V_\text{O}>V_\text{N}>V_\text{H}\)
4. \(V_\text{O}>V_\text{H}>V_\text{N}\)
Molecular weight of two gases are \(M_1\) and \(M_2.\) At any temperature, the ratio of root mean square velocities \(v_1\) and \(v_2\) will be:
1. \(\sqrt{\frac{M_1}{M_2}}\)
2. \(\sqrt{\frac{M_2}{M_1}}\)
3. \(\sqrt{\frac{M_1+M_2}{M_1-M_2}}\)
4. \(\sqrt{\frac{M_1-M_2}{M_1+M_2}}\)
The root mean square velocity of the molecules of a gas is 300 m/s. What will be the root mean square speed of the molecules if the atomic weight is doubled and absolute temperature is halved?
1. | 300 m/s | 2. | 150 m/s |
3. | 600 m/s | 4. | 75 m/s |
The molecules of a given mass of gas have rms velocity of 200 ms-1 at \(27^{\circ}\mathrm{C}\) and 1.0 x 105 Nm-2 pressure. When the temperature and pressure of the gas are increased to, respectively, \(127^{\circ}\mathrm{C}\) and 0.05 X 105 Nm-2, rms velocity of its molecules in ms-1 will become:
1. 400/√3
2. 100√2/3
3. 100/3
4.100√2
If the ratio of vapour density for hydrogen and oxygen is \(1 \over 16\), then under constant pressure, the ratio of their rms velocities will be:
1. | \(4 \over 1\) | 2. | \(1 \over 4\) |
3. | \(1 \over 16\) | 4. | \(16 \over 1\) |
At which temperature the velocity of \(\mathrm{O_2}\) molecules will be equal to the velocity of \(\mathrm{N_2}\) molecules at \(0^\circ \mathrm{C}?\)
1. | \(40^\circ \mathrm{C}\) | 2. | \(93^\circ \mathrm{C}\) |
3. | \(39^\circ \mathrm{C}\) | 4. | Cannot be calculated |
The rms speed of the molecules of an enclosed gas is \(v\). What will be the rms speed if the pressure is doubled, keeping the temperature constant?
1. | \(v \over 2\) | 2. | \(v\) |
3. | \(2v\) | 4. | \(4v\) |
A. | \((\overline{v^2})\). | They have an equal mean square velocity
B. | \((\overline{v^2})\) than an oxygen molecule. | A nitrogen molecule has a greater mean square velocity
C. | A nitrogen molecule has a greater mean kinetic energy than an oxygen molecule. |
D. | An oxygen molecule has a greater mean kinetic energy than a nitrogen molecule. |
Uranium has two isotopes of masses \(235 \) and \(238\) units. If both are present in Uranium hexafluoride gas, which would have the larger average speed?
1. \(^{235} \mathrm{U} \mathrm{F}_{6}\)
2. \({}^{238} \mathrm{U} \mathrm{F}_{6}\)
3. Both will have the same average speed.
4. Data insufficient
The curve between absolute temperature and \(\mathrm{v}^2_{rms}\) is:
1. | 2. | ||
3. | 4. |