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 rms speed of oxygen atoms is v. If the temperature is halved and the oxygen atoms combine to form oxygen molecules, then the rms speed will be:
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3. 2v
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Two thermally insulated vessels \(1\) and \(2\) are filled with air at temperatures \(\mathrm{T_1},\) \(\mathrm{T_2},\) volume \(\mathrm{V_1},\) \(\mathrm{V_2}\) and pressure \(\mathrm{P_1},\) \(\mathrm{P_2}\) respectively. If the valve joining the two vessels is opened, the temperature inside the vessel at equilibrium will be:
1. | \(T_1+T_2\) | 2. | \(\dfrac{T_1+T_2}{2}\) |
3. | \(\dfrac{T_1T_2(P_1V_1+P_2V_2)}{P_1V_1T_2+P_2V_2T_1}\) | 4. | \(\dfrac{T_1T_2(P_1V_1+P_2V_2)}{P_1V_1T_1+P_2V_2T_2}\) |
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. \(V_\text{O}>V_\text{H}>V_\text{N}\)
If the mean free path of atoms is doubled , then the pressure of the gas will become:
1. P/4
2. P/2
3. P/8
4. P
The relation between two specific heats (in cal/mol) of a gas is:
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The pressure in a diatomic gas increases from to , when its volume is increased from . The increase in internal energy will be:
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In the PV graph shown below for an ideal diatomic gas, the change in the internal energy is:
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The figure shows a process for a gas in which pressure (P) and volume (V) of the gas change. If and are the molar heat capacities of the gas during the processes AB and BC respectively, then:
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