The van der Waals equation of gas is - P-n2a-V2 -V-nb-nRT-

The correct option is A TrueTrue, #160;The van der Waals equation of gas is [ P+n^2a/V^2 ](V nb)=nRT .It is applicable to real and ideal gases. For real ...

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Standard XII

Chemistry

Liquefaction of Gases and Critical Constants

The van der W...

Question

The van der Waals equation of gas is $[P + \frac{n^{2} a}{V^{2}}] (V - n b) = n R T$ .

True

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False

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Solution

The correct option is A True
True,
The van der Waals equation of gas is $[P + \frac{n^{2} a}{V^{2}}] (V - n b) = n R T$ .
It is applicable to real and ideal gases. For real gases constants $a$ and $b$ have same value. For ideal gas $a = 0, b = 0.$

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Similar questions

Q. In the van der Waals equation

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

constant

a

reflects the actual volume of the gas molecules.

Q. In the van der Waals equation given below,

(p + \frac{a n}{V^{2}}) (V - n b) = n R T,

the

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

and

n b

terms represent, respectively, corrections for:

Q. Van der Waal's equation for a gas is stated as,

p = \frac{n R T}{V - n b} - a (\frac{n}{b})^{2}

. This equation reduces to the perfect gas equation,

p = \frac{n R T}{V}

, when _____________.

Q. Given, Van der waals equation for non-ideal gas

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

The term that correctly describes intermolecular forces of attraction between the molecules is:

State True or False.

In the van der Waal's equation,

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

the constant '

a

' reflects the actual volume of the gas molecules.

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The van der Waals equation of gas is [P+n2aV2](V−nb)=nRT.

The correct option is A TrueTrue, The van der Waals equation of gas is [P+n2aV2](V−nb)=nRT.It is applicable to real and ideal gases. For real gases constants a and b have same value. For ideal gas a=0,b=0.

The van der Waals equation of gas is $[P + \frac{n^{2} a}{V^{2}}] (V - n b) = n R T$ .

The correct option is A True
True,
The van der Waals equation of gas is $[P + \frac{n^{2} a}{V^{2}}] (V - n b) = n R T$ .
It is applicable to real and ideal gases. For real gases constants $a$ and $b$ have same value. For ideal gas $a = 0, b = 0.$