(A) According to the ideal gas equation,we have: $PV = nRT$ Since the number of moles $n = \frac{m}{M}$,where $m$ is the mass and $M$ is the molar mas

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(A) According to the ideal gas equation,we have: $PV = nRT$ Since the number of moles $n = \frac{m}{M}$,where $m$ is the mass and $M$ is the molar mass,we can substitute this into the equation: $PV = \frac{m}{M} RT$ Rearranging the terms to solve for density $\rho = \frac{m}{V}$: $P = \frac{m}{V} \times \frac{RT}{M}$ $P = \rho \times \frac{RT}{M}$ Therefore,the density $\rho$ is given by: $\rho = \frac{PM}{RT}$

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

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The density of an ideal gas can be given by where $P$,$V$,$M$,$T$ and $R$ respectively denote pressure,volume,molar mass,temperature and universal gas constant.

AP EAMCET 2021 All AP EAMCET

A
$\frac{PM}{RT}$
B
$\frac{PV}{RT}$
C
$\frac{RT}{PM}$
D
$\frac{RT}{PV}$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

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The density of a gas at $-23 \ ^oC$ temperature and $780 \ \text{torr}$ pressure is $1.40 \ g/L$. Identify the gas.

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If $R = 8.314$,express it with its units.

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The density of an ideal gas can be given by where $P$,$V$,$M$,$T$ and $R$ respectively denote pressure,volume,molar mass,temperature and universal gas constant.

Similar Questions

Find the pressure of a $CO_2$ gas when $6.022 \times 10^{22}$ molecules are placed in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

At what temperature in the Celsius scale,$V$ (volume) of a certain mass of gas at $27\,^oC$ will be doubled keeping the pressure constant?

The density of a gas at $-23 \ ^oC$ temperature and $780 \ \text{torr}$ pressure is $1.40 \ g/L$. Identify the gas.

The temperature at which $4 \ mol$ of a gas occupies $5 \ dm^3$ volume at $3.32 \ bar$ pressure is:

If $R = 8.314$,express it with its units.

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