During an experiment, an ideal gas is found to obey an additional law VP2 = constant. The gas is initially at temperature T and volume V. What will be the temperature of the gas when it expands to a volume 2V?
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We have two vessels of equal volume, one filled with hydrogen and the other with equal mass of helium. The common temperature is \(27^{\circ}\mathrm{C}\) . What is the relative number of molecules in the two vessels?
1. \(\frac{n_H}{n_{He}} = \frac{1}{1}\)
2. \(\frac{n_H}{n_{He}} = \frac{5}{1}\)
3. \(\frac{n_H}{n_{He}} = \frac{2}{1}\)
4. \(\frac{n_H}{n_{He}} = \frac{3}{1}\)
The volume \(V\) versus temperature \(T\) graph for a certain amount of a perfect gas at two pressures \(\mathrm{P}_1\) and
\(\mathrm{P}_2\) are shown in the figure. Here:
1. | \(\mathrm{P}_1<\mathrm{P}_2\) |
2. | \(\mathrm{P}_1>\mathrm{P}_2\) |
3. | \(\mathrm{P}_1=\mathrm{P}_2\) |
4. | Pressures can’t be related |
At a pressure of 24 × 105 dyne/cm2, the volume of O2 is 10 litre and mass is 20g. The rms velocity will be:
1. | 800 m/s | 2. | 400 m/s |
3. | 600 m/s | 4. | Data is incomplete |
The value of for a gas in state A and in another state B. If denote the pressure and denote the temperatures in the two states, then:
1. | \(P_A=P_B ; T_A>T_B\) |
2. | \(P_A>P_B ; T_A=T_B\) |
3. | \(P_A<P_B ; T_A>T_B\) |
4. | \(P_A=P_B ; T_A<T_B\) |
The volume and temperature graph is given in the figure below. If pressures for the two processes are different, then which one, of the following, is true?
1. | \(P_1=P_2\) and \(P_3=P_4\) and \(P_3>P_2\) |
2. | \(P_1=P_2\) and \(P_3=P_4\) and \(P_3<P_2\) |
3. | \(P_1=P_2\) \(=\) \(P_3=P_4\) |
4. | \(P_1>P_2\) \(>\) \(P_3>P_4\) |
At \(10^{\circ}\mathrm{C}\) the value of the density of a fixed mass of an ideal gas divided by its pressure is \(x\). At \(110^{\circ}\mathrm{C}\) this ratio is:
1. | \(x\) | 2. | \(\dfrac{383}{283}x\) |
3. | \(\dfrac{10}{110}x\) | 4. | \(\dfrac{283}{383}x\) |
The amount of heat energy required to raise the temperature of \(1\) g of Helium at NTP, from \({T_1}\) K to \({T_2}\) K is:
1. \(\frac{3}{2}N_ak_B(T_2-T_1)\)
2. \(\frac{3}{4}N_ak_B(T_2-T_1)\)
3. \(\frac{3}{4}N_ak_B\frac{T_2}{T_1}\)
4. \(\frac{3}{8}N_ak_B(T_2-T_1)\)
One mole of an ideal diatomic gas undergoes a transition from \(A\) to \(B\) along a path \(AB\) as shown in the figure.
The change in internal energy of the gas during the transition is:
1. | \(20\) kJ | 2. | \(-20\) kJ |
3. | \(20\) J | 4. | \(-12\) kJ |