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NEET Practice Questions (MCQs) with Answers & Solutions

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A gas is filled in a cylinder, its temperature is incresecd by 20% on kelvin scale and volume is reduced by 10%. How much percentage of the gas will leak out

A. 15% B. 25% C. 40% D. 30%

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Explanation

Let initial conditions = V, T final conditions = V', T' By Charle's law, $ V \alpha T $ ( P remains constant ) But as per question, volume is reduced by 10% means Therefore V' = 0.9 V so percentage of volume leaked out $= { (1.2 - 0.9 ) V \over 1.2 V } \times 100 \% = 25 \% $

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The pressure is exerted by the gas on the walls of the container because

A. It sticks with the walls B. It is accelerated towards the walls C. It loses kinetic energy D. On collision with the walls there is a change in momentum

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Explanation

$ Pressure P = { F \over A } = { 1 \over A } { \triangle P \over \triangle t } $ $ ( \triangle P = change in momentum) $

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The relation between the gas pressure P and average kinetic energy per unit volume E is

A. P = 2 /3 E B. P = 3/2 E C. P = E D. P = E / 2

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Explanation

$$ P = {2 \over 3 } ( Energy per unit volume ) $$ $$ = { 2 \over 3 } { E \over V } = { 2 \over 3 } E $$

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The root mean square speed of hydrogen molecules of an ideal hydrogen kept in a gas chamber at $ 0 ^\circ C$ is $ 3180 ms^{â€“1} $. The pressure on the hydrogen gas is $ (Density of hydrogen gas is 8.99 \times 10^{-2} kg/ m3 , 1 atm = 1.01 \times 10^5 Nm^{-2 } ) $

A. 1.0 atm B. 3.0 atm C. 2.0 atm D. 1.5 atm

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Explanation

$ V_{rms} = \sqrt { 3P \over \rho } \Rightarrow P = { V^2 _ {rms } \rho \over 3 } $

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Gas at a pressure $P_o$ is contained in a vessel. If the masses of all the molecules are halved and their speeds are doubled, the resulting pressure will be equal to

A. $ 2 P_o $ B. $ 4 P_o $ C. $ P_o /2 $ D. $ P_o $

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Explanation

$ V _{rms } = \sqrt { 3P \over \rho} = \sqrt { 3PV \over M } \Rightarrow V_{rms } \alpha \sqrt { P \over M } $ $ \therefore{ V_1 \over V_2 }= \sqrt { {P_1 \over P_2 } \times { M_2 \over M_1 }} $

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A cylinder of capacity 20 litres is filled with $H_2$ gas. The total average kinetic energy of translatory motion of its molecules is $1.5 \times 10^5 J $. The pressure of hydrogen in the cylinder is

A. $ 4 \times 10^6 Nm^{-2} $ B. $ 3 \times 10^6 Nm^{-2} $ C. $ 5 \times 10^6 Nm^{-2} $ D. $ 2 \times 10^6 Nm^{-2} $

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Explanation

$ E = { 3 \over 2 } PV \Rightarrow P = { 2 E \over 3V } $

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The average kinetic energy per molecule of a gas at $ -23 ^\circ C$ and 75 cm pressure is $ 5 \times 10^{-14} $ erg for $H_2$ . The mean kinetic energy per molecule of the $O_2$ at $ 227 ^\circ C $ and 150 cm pressure will be

A. $ 80 \times 10^{-14}erg $ B. $ 10 \times 10^{-14}erg $ C. $ 20 \times 10^{-14}erg $ D. $ 40 \times 10^{-14}erg $

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Explanation

The average kinetic energy $ E = { 3 \over 2 } k_B T $ $ \therefore { E_1 \over E_2 } = { T_1 \over T_2 } $

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The ratio of mean kinetic energy of hydrogen and oxygen at a given temperature is

A. 1:8 B. 1:4 C. 1:16 D. 1:1

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Explanation

Kinetic energy is a function of temperature.

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The ratio of mean kinetic energy of hydrogen and nitrogen at temperature 300 K and 450 K respectively is

A. 2:3 B. 3:2 C. 1:16 D. 2:2

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Explanation

$ E \alpha T $ $ \therefore { E_1 \over E_2 } = { T_1 \over T_2 } $

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Pressure of an ideal gas is increased by keeping temperature constant what is the effect on kinetic energy of molecules.

A. Decrease B. Increase C. No change D. Can't be determined

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Explanation

Kinetic energy of ideal gas depends only on its temperature. Hence, it remains constant whether pressure is increased or decreased.

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