(B) Using the ideal gas equation $PV = nRT$, where $n = \frac{m}{M}$.Given: $P = 760 \text{ mm of Hg} = 1 \text{ atm}$, $V = 11.2 \text{ litres}$, $T

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(B) Using the ideal gas equation $PV = nRT$, where $n = \frac{m}{M}$.Given: $P = 760 \text{ mm of Hg} = 1 \text{ atm}$, $V = 11.2 \text{ litres}$, $T = 27^{\circ}C = 300 \text{ K}$, $M = 32 \text{ g/mol} = 0.032 \text{ kg/mol}$, $R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1}$.$m = \frac{PVM}{RT} = \frac{1 \times 11.2 \times 32}{0.0821 \times 300} \text{ grams}$.$m \approx 14.56 \text{ grams} = 0.01456 \text{ kg}$.

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

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The mass of oxygen gas occupying a volume of $11.2 \text{ litres}$ at a temperature $27^{\circ}C$ and a pressure of $760 \text{ mm}$ of mercury in kilograms is $[$ Molecular weight of oxygen $= 32]$

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AP EAMCET 2002 All AP EAMCET

A
$0.001456$
B
$0.01456$
C
$0.1456$
D
$1.1456$

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Class 11

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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

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Pressure of a gas of constant volume at $20^{\circ} C$ is $90 \ cm$ of $Hg$. At what temperature the pressure would change to $75 \ cm$ of $Hg$ (in $^{\circ} C$)?

EasyAP EAMCET 2020

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What does the universal gas constant $R$ represent? Write its value and unit.

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The mass of oxygen gas occupying a volume of $11.2 \text{ litres}$ at a temperature $27^{\circ}C$ and a pressure of $760 \text{ mm}$ of mercury in kilograms is $[$ Molecular weight of oxygen $= 32]$

Similar Questions

For an ideal gas with pressure $P$,temperature $T$,and volume $V$,where the mass of each molecule is $m$,what is the density of the gas? ($k$ is the Boltzmann constant)

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