For real gases- the relation between P- V and T is given by van der Waals equation- P - an2V2 V - nb - nRT- For the following gases CH4- CO2- O2- H2 which gas will have i highest value of a ii- lowest value of b-

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Standard XII

Chemistry

Real Gases

For real gase...

Question

For real gases, the relation between $P, V$ and $T$ is given by van der Waals equation, $(P + \frac{a n^{2}}{V^{2}}) (V - n b) = n R T$ . For the following gases $C H_{4}, C O_{2}, O_{2}, H_{2}$ which gas will have (i) highest value of $a$ (ii), lowest value of $b$ ?

(i)

C O_{2}

, (ii)

H_{2}

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(i)

C H_{4}

, (ii)

C O_{2}

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(i)

H_{2}

, (ii)

C O_{2}

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(i)

O_{2}

, (ii)

H_{2}

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Solution

The correct option is A (i) $C O_{2}$ , (ii) $H_{2}$
(i) Order of intermolecular attraction is $C O_{2} > C H_{4} > O_{2} > H_{2}$
In $C O_{2}$ , intermolecular forces increases with number of electrons in a molecule.
(ii) Size increases in order of $H_{2} < O_{2} < C H_{4} < C O_{2}$
Hence, $H_{2}$ will have lowest value of $b$ .

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

where 'a' and 'b' are van der Waals' constants, 'nb' is approximately equal to the total volume of the molecules of a gas. 'a' is the measure of the magnitude of intermolecular attraction.

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For real gases, the relation between P,V and T is given by van der Waals equation, (P+an2V2)(V−nb)=nRT. For the following gases CH4,CO2,O2,H2 which gas will have (i) highest value of a (ii), lowest value of b?

The correct option is A (i) CO2, (ii) H2(i) Order of intermolecular attraction is CO2>CH4>O2>H2In CO2, intermolecular forces increases with number of electrons in a molecule.(ii) Size increases in order of H2<O2<CH4<CO2Hence, H2 will have lowest value of b.

For real gases, the relation between $P, V$ and $T$ is given by van der Waals equation, $(P + \frac{a n^{2}}{V^{2}}) (V - n b) = n R T$ . For the following gases $C H_{4}, C O_{2}, O_{2}, H_{2}$ which gas will have (i) highest value of $a$ (ii), lowest value of $b$ ?