(B) The van der Waals gas equation for $1 \ mol$ of gas is $(P + \frac{a}{V^2})(V - b) = RT$. At low pressure,the volume $V$ is very large,so $V - b \

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(B) The van der Waals gas equation for $1 \ mol$ of gas is $(P + \frac{a}{V^2})(V - b) = RT$. At low pressure,the volume $V$ is very large,so $V - b \approx V$. Substituting this into the equation: $(P + \frac{a}{V^2})V = RT$. Expanding the terms: $PV + \frac{a}{V} = RT$. Rearranging gives: $PV = RT - \frac{a}{V}$.

Class 11 Chemistry States of Matter Real gases and Vander waal’s equation

Medium

The van der Waals equation for $CH_4$ at low pressure is:

A
$PV = RT - Pb$
B
$PV = RT - \frac{a}{V}$
C
$PV = RT + \frac{a}{V}$
D
$PV = RT + Pb$

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Class 11

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States of Matter

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Real gases and Vander waal’s equation

At $300 \, K$ temperature and $40 \, atm$ pressure,if one mole of $CO_2$ occupies $0.4 \, L$,then it is:

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Calculate the compressibility factor $Z$ for $CO_2$,if one mole of it occupies $0.4 \ L$ at $300 \ K$ and $40 \ atm$. Also,comment on the result.

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What is the difference in the pressure-volume $(P-V)$ graph (at constant $T$) for a real gas and an ideal gas?

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Which of the following represents the $Van \ der \ Waals$ equation for $n$ moles of a real gas?

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The compressibility factor $Z = \frac{pV}{nRT}$ for hydrogen gas at $273 \ K$ and $1 \ atm$ pressure is

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The van der Waals equation for $CH_4$ at low pressure is:

Similar Questions

At $300 \, K$ temperature and $40 \, atm$ pressure,if one mole of $CO_2$ occupies $0.4 \, L$,then it is:

Calculate the compressibility factor $Z$ for $CO_2$,if one mole of it occupies $0.4 \ L$ at $300 \ K$ and $40 \ atm$. Also,comment on the result.

What is the difference in the pressure-volume $(P-V)$ graph (at constant $T$) for a real gas and an ideal gas?

Which of the following represents the $Van \ der \ Waals$ equation for $n$ moles of a real gas?

The compressibility factor $Z = \frac{pV}{nRT}$ for hydrogen gas at $273 \ K$ and $1 \ atm$ pressure is

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