(C) According to Boyle's law,for a constant temperature,$P_{1}V_{1} = P_{2}V_{2}$.Given:Initial pressure at $N.T.P.$,$P_{1} = 76 \ cm$ of $Hg$.Initial

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(C) According to Boyle's law,for a constant temperature,$P_{1}V_{1} = P_{2}V_{2}$.Given:Initial pressure at $N.T.P.$,$P_{1} = 76 \ cm$ of $Hg$.Initial volume,$V_{1} = 5 \ L$.Final volume,$V_{2} = 5 \ L + 30 \ L = 35 \ L$.Applying the formula:$76 \times 5 = P_{2} \times 35$$P_{2} = \frac{76 \times 5}{35}$$P_{2} = \frac{76}{7} \approx 10.857 \ cm$ of $Hg$.Rounding to two decimal places,the resultant pressure is $10.86 \ cm$ of $Hg$. The closest option is $10.85 \ cm$ of $Hg$.

Class 11 Physics Kinetic Theory of Gases Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

Medium

$A$ cylinder of $5 \ L$ capacity,filled with air at $N.T.P.$,is connected to another evacuated cylinder of $30 \ L$ capacity. The resultant air pressure in both the cylinders will be ...... $cm$ of $Hg$. (in $.85$)

A
$38$
B
$21$
C
$10$
D
$14$

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Kinetic Theory of Gases

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Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

Air pressure in a car tyre increases during driving. Explain.

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The gas equation $\frac{PV}{T} = \text{constant}$ is true for a constant mass of an ideal gas undergoing:

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You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen?

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When a gas in a closed vessel was heated so as to increase its temperature by $5^{\circ}C$,there occurred an increase of $1\%$ in its pressure. The original temperature of the gas was ...... $^{\circ}C$

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In the given $(V - T)$ diagram,what is the relation between pressures $P_1$ and $P_2 \,?$

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$A$ cylinder of $5 \ L$ capacity,filled with air at $N.T.P.$,is connected to another evacuated cylinder of $30 \ L$ capacity. The resultant air pressure in both the cylinders will be ...... $cm$ of $Hg$. (in $.85$)

Similar Questions

Air pressure in a car tyre increases during driving. Explain.

The gas equation $\frac{PV}{T} = \text{constant}$ is true for a constant mass of an ideal gas undergoing:

You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen?

When a gas in a closed vessel was heated so as to increase its temperature by $5^{\circ}C$,there occurred an increase of $1\%$ in its pressure. The original temperature of the gas was ...... $^{\circ}C$

In the given $(V - T)$ diagram,what is the relation between pressures $P_1$ and $P_2 \,?$

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