At low pressure- van der Waal-s equation for 1 mol can be represented asA- Z-1-a-V R TB- Z-a-V R TC - Z -1-a-V R T- Z -V R T-a

The correct option is C (P+a/V^2 )(V b)=RT At low P, volume is very large . ∴ “b” can be ignored. (P+a/V^2 )V=RT PV+a/v=RT (Divide the equation by RT) PV ...

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Standard XII

Chemistry

Real Gases

At low pressu...

Question

At low pressure, van der Waal’s equation for 1 mol can be represented as

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Solution

The correct option is B

$(P + \frac{a}{V^{2}}) (V - b) = R T$

At low P, volume is very large . $∴$ “b” can be ignored.

$(P + \frac{a}{V^{2}}) V = R T$

$P V + \frac{a}{v} = R T$ (Divide the equation by RT)

$\frac{P V}{R T} + \frac{a}{R T V} = 1$

$∴ Z = 1 - \frac{a}{V R T} (\frac{P V}{R T} = Z f o r 1 m o l)$

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Similar questions

Q. If

Z

is a compresibility factor, van der waals equation at low pressure can be written as:

Q. If

Z

is a compressibility factor, van der Waals equation at low pressure can be written as :

Q. Assertion :The increase in compressibility factor with increasing pressure is due to

a

. Reason:

Z = 1 + \frac{b P}{R T}

for real gases can be obtained by neglecting

\frac{a}{V^{2}}

term in van der Waal's equation.

Q. Van der Waal's equation at high pressure for

1 m o l e

is:

Q. Assertion :Compressibility factor Z according to van der Waal's equation may be written as

Z = \frac{1}{1 - (\frac{n b}{V})} - \frac{a n}{R T V}

. Reason: For real gases

Z >< 1

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At low pressure, van der Waal’s equation for 1 mol can be represented as

The correct option is B (P+aV2)(V−b)=RT At low P, volume is very large . ∴ “b” can be ignored. (P+aV2)V=RT PV+av=RT (Divide the equation by RT) PVRT+aRTV=1 ∴ Z=1−aVRT(PVRT=Z for 1 mol)