(C) From the ideal gas equation,$PV = nRT$,we know $PV = (m/M)RT$,where $m$ is mass and $M$ is molar mass.Rearranging for density $d = m/V$,we get $d

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(C) From the ideal gas equation,$PV = nRT$,we know $PV = (m/M)RT$,where $m$ is mass and $M$ is molar mass.Rearranging for density $d = m/V$,we get $d = PM/RT$.Thus,$P = dRT/M$.Given $d_x = 2d_y$ and $M_y = 3M_x$.The ratio of pressures is $\frac{P_x}{P_y} = \frac{d_x R T / M_x}{d_y R T / M_y} = \frac{d_x}{d_y} \times \frac{M_y}{M_x}$.Substituting the given values: $\frac{P_x}{P_y} = (2) \times (3) = 6$.

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

Medium

At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

A
$0.25$
B
$4$
C
$6$
D
$1/6$

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States of Matter

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Ideal gas equation and Related gas laws

According to Boyle's law,what are the two isothermal graphs and what is their nature?

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At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

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Under what conditions does an ideal gas have maximum density?

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An ideal gas expands isothermally and reversibly from $10 \ m^3$ to $20 \ m^3$ at $300 \ K$,performing $5.187 \ kJ$ of work on the surroundings. Calculate the number of moles of gas used.

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At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

Similar Questions

According to Boyle's law,what are the two isothermal graphs and what is their nature?

How many moles of $He$ gas occupy $22.4 \, L$ at $30^{\circ}C$ and $1 \, atm$ pressure?

At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

Under what conditions does an ideal gas have maximum density?

An ideal gas expands isothermally and reversibly from $10 \ m^3$ to $20 \ m^3$ at $300 \ K$,performing $5.187 \ kJ$ of work on the surroundings. Calculate the number of moles of gas used.

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