(B) Using the ideal gas equation $PV = nRT$,where $n = \frac{m}{M}$ and $d = \frac{m}{V}$,we get $P = \frac{dRT}{M}$.Rearranging for molar mass: $M =

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(B) Using the ideal gas equation $PV = nRT$,where $n = \frac{m}{M}$ and $d = \frac{m}{V}$,we get $P = \frac{dRT}{M}$.Rearranging for molar mass: $M = \frac{dRT}{P}$.Given values:$d = 0.46 \, g \, L^{-1}$$R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$$T = 257 + 273 = 530 \, K$$P = \frac{100}{760} \, atm$Substituting these values:$M = \frac{0.46 \times 0.082 \times 530 \times 760}{100}$$M = 151.93 \, g \, mol^{-1}$.Rounding to the nearest integer,we get $152$.

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

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Geraniol,a volatile organic compound,is a component of rose oil. The density of the vapour is $0.46 \, g \, L^{-1}$ at $257^{\circ} C$ and $100 \, mm \, Hg$. The molar mass of geraniol is $....$ (Nearest Integer) [Given $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$]

JEE MAIN 2022 All JEE MAIN

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$89$
B
$152$
C
$741$
D
$236$

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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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At $1 \text{ atm}$ pressure and $0 \, ^oC$,a certain mass of a gas occupies $0.4 \, L$. Keeping the pressure constant,if the temperature is increased to $273 \, ^oC$,what will be its final volume (in $, L$)?

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At constant temperature and pressure,what is the volume of $n$ moles of different gases?

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Geraniol,a volatile organic compound,is a component of rose oil. The density of the vapour is $0.46 \, g \, L^{-1}$ at $257^{\circ} C$ and $100 \, mm \, Hg$. The molar mass of geraniol is $....$ (Nearest Integer) [Given $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$]

Similar Questions

The density of oxygen gas at $5 \text{ atm}$ and $127^{\circ} C$ will be (in $\text{ g/L}$)

If pressure becomes double at the same absolute temperature on $2 \ L$ $CO_2$,then the volume of $CO_2$ becomes ............ $L$.

If $2$ moles of an ideal gas at $546 \ K$ has a volume of $44.8 \ L$,then what will be its pressure (in $atm$)? $(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

At $1 \text{ atm}$ pressure and $0 \, ^oC$,a certain mass of a gas occupies $0.4 \, L$. Keeping the pressure constant,if the temperature is increased to $273 \, ^oC$,what will be its final volume (in $, L$)?

At constant temperature and pressure,what is the volume of $n$ moles of different gases?

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