Q. No.A container has two chambers of volumes \(V_1=2~\text{litres} \) and \(V_2=3~\text{litres} \) separated by a partition made of a thermal insulator. The chambers contains \( n_1=5 \) and \( n_2=4 \) moles of ideal gas at pressures \(p_1=1~\text{atm} \) and \(p_2=2~\text{atm}, \) respectively. When the partition is removed, the mixture attains an equilibrium pressure of:
| 1. | \(1.4 ~\text{atm} \) | 2. | \(1.8 ~\text{atm} \) |
| 3. | \(1.3 ~\text{atm} \) | 4. | \(1.6 ~\text{atm} \) |
Subtopic: Ideal Gas Equation |
Level 3: 35%-60%
NEET - 2025
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An oxygen cylinder of volume \(30\) litre has \(18.20\) moles of oxygen. After some oxygen is withdrawn from the cylinder, its gauge pressure drops to \(11\) atmospheric pressure at temperature \(27^{\circ} \text{C}.\) The mass of the oxygen withdrawn from the cylinder is nearly equal to:
\([\)Given, \(R=\frac{100}{12}~ \text{J} \mathrm{~mol}^{-1} {~\text K}^{-1},\) and molecular mass of \(O_2=32,\) \(1\) atm pressure \(\left.=1.01 \times 10^5 \mathrm{~N} / \mathrm{m}\right]\)
1. \(0.116\text{ kg}\)
2. \(0.156\text{ kg}\)
3. \(0.125\text{ kg}\)
4. \(0.144\text{ kg}\)
\([\)Given, \(R=\frac{100}{12}~ \text{J} \mathrm{~mol}^{-1} {~\text K}^{-1},\) and molecular mass of \(O_2=32,\) \(1\) atm pressure \(\left.=1.01 \times 10^5 \mathrm{~N} / \mathrm{m}\right]\)
1. \(0.116\text{ kg}\)
2. \(0.156\text{ kg}\)
3. \(0.125\text{ kg}\)
4. \(0.144\text{ kg}\)
Subtopic: Ideal Gas Equation |
Level 4: Below 35%
NEET - 2025
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The following graph represents the \(T\text -V\) curves of an ideal gas (where \(T\) is the temperature and \(V\) the volume) at three pressures \(P_1, P_2\) and \(P_3\) compared with those of Charles's law represented as dotted lines.
Then the correct relation is:
Then the correct relation is:
| 1. | \(P_1>P_3>P_2 \) | 2. | \(P_2>P_1>P_3 \) |
| 3. | \( P_1>P_2>P_3\) | 4. | \(P_3 > P_2>P_1\) |
Subtopic: Ideal Gas Equation |
67%
Level 2: 60%+
NEET - 2024
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An ideal gas at \(0^{\circ}\text{C}\) and atmospheric pressure \(P\) has volume \(V.\) The percentage increase in its temperature needed to expand it to \(3V\) at constant pressure is:
| 1. | \(100\%\) | 2. | \(200\%\) |
| 3. | \(300\%\) | 4. | \(50\%\) |
Subtopic: Ideal Gas Equation |
69%
Level 2: 60%+
NEET - 2024
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A container of volume \(200\) cm3 contains \(0.2\) mole of hydrogen gas and \(0.3\) mole of argon gas. The pressure of the system at temperature \(200\) K (\(R=8.3\) JK–1 mol–1) will be:
| 1. | \( 6.15 \times 10^5 ~\text{Pa} \) | 2. | \( 6.15 \times 10^4 ~\text{Pa} \) |
| 3. | \( 4.15 \times 10^5 ~\text{Pa} \) | 4. | \( 4.15 \times 10^6 ~\text{Pa}\) |
Subtopic: Ideal Gas Equation |
61%
Level 2: 60%+
NEET - 2023
Hints
The volume occupied by the molecules contained in \(4.5~\text{kg}\) water at STP, if the molecular forces vanish away, is:
| 1. | \(5.6~\text{m}^3\) | 2. | \(5.6\times10^{6}~\text{m}^3\) |
| 3. | \(5.6\times10^{3}~\text{m}^3\) | 4. | \(5.6\times10^{-3}~\text{m}^3\) |
Subtopic: Ideal Gas Equation |
Level 3: 35%-60%
NEET - 2022
Hints
A cylinder contains hydrogen gas at a pressure of \(249~\text{kPa}\) and temperature \(27^\circ\text{C}.\) Its density is:
(\(R=8.3~\text{J mol}^{-1} \text {K}^{-1}\))
1. \(0.2~\text{kg/m}^{3}\)
2. \(0.1~\text{kg/m}^{3}\)
3. \(0.02~\text{kg/m}^{3}\)
4. \(0.5~\text{kg/m}^{3}\)
Subtopic: Ideal Gas Equation |
63%
Level 2: 60%+
NEET - 2020
Hints
Links
An ideal gas equation can be written as \(P = \dfrac{ρRT}{M_{0}}\) where \(\rho\) and \(M_{0}\) are respectively:
| 1. | mass density, the mass of the gas. |
| 2. | number density, molar mass. |
| 3. | mass density, molar mass. |
| 4. | number density, the mass of the gas. |
Subtopic: Ideal Gas Equation |
79%
Level 2: 60%+
NEET - 2020
Hints
A given sample of an ideal gas occupies a volume \(V\) at a pressure \(P\) and absolute temperature \(T\). The mass of each molecule of the gas is \(m\). Which of the following gives the density of the gas?
| 1. | \(\dfrac{P}{kT}\) | 2. | \(\dfrac{Pm}{kT}\) |
| 3. | \(\dfrac{P}{kTV}\) | 4. | \(mkT\) |
Subtopic: Ideal Gas Equation |
86%
Level 1: 80%+
NEET - 2016
Hints
Two vessels separately contain two ideal gases \(A\) and \(B\) at the same temperature, the pressure of \(A\) being twice that of \(B.\) Under such conditions, the density of \(A\) is found to be \(1.5\) times the density of \(B.\) The ratio of molecular weight of \(A\) and \(B\) is:
| 1. | \(\dfrac{2}{3}\) | 2. | \(\dfrac{3}{4}\) |
| 3. | \(2\) | 4. | \(\dfrac{1}{2}\) |
Subtopic: Ideal Gas Equation |
87%
Level 1: 80%+
NEET - 2015
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