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Van der Waal's Forces

'a' and 'b' a...

Question

'a' and 'b' are van der Waals' constants for gases. Chlorine is more easily liquefied than ethane because

a and b for

C l_{2} > a

and b for

C_{2} H_{6}

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a and b for

C l_{2} < a

and b for

C_{2} H_{6}

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a for

C l_{2} > a

for

C_{2} H_{6}

but b for

C l_{2} > b

for

C_{2} H_{6}

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a for

C l_{2} > a

for

C_{2} H_{6}

but b for

C l_{2} < b

for

C_{2} H_{6}

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Solution

The correct option is D a for $C l_{2} > a$ for $C_{2} H_{6}$ but b for $C l_{2} < b$ for $C_{2} H_{6}$
The value of $^{'} a^{'}$ is a measure of the magnitude of the attractive forces between the molecules of the gas. Greater the value of 'a', larger is the attractive intermolecular force between the gas molecules.
The value of 'b' related to the effective size of the gas molecules. It is also termed as excluded volume.
The gases with higher value of 'a' and lower value of 'b' are more liquefiable, hence for $C l_{2}$ 'a' should be greater than for $C_{2} H_{6}$ but for it 'b' should be less than for $C_{2} H_{6}$ .

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a

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Chlorine is more easily liquefied than ethane because ("a” and "b" are van der waals constants for gases).

^{'} a^{'}

^{'} b^{'}

^{'} a^{'}

^{'} b^{'}

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