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Byju's Answer

Standard XII

Chemistry

Real Gases

For real gase...

Question

For real gases van der Waals equation is written as
$(P + \frac{a n^{2}}{V^{2}}) (V - n b) = n R T$
Where 'a' and 'b' are van der Waals constants.
Two sets of gases are :
(I) $O_{2}, C O_{2}, H_{2}$ and He (II) $C H_{4}, O_{2} a n d H_{2}$
The gases given in set-I in increasing order of 'b' and gases given in set-II in decreasing order of 'a' are arranged below. Select the correct order from the following:

(I) O_{2} < H e < H_{2} < C O_{2} (I I) H_{2} > O_{2} > C H_{4}

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(I) H_{2} < H e < O_{2} < C O_{2} (I I) C H_{4} > O_{2} > H_{2}

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(I) H_{2} < O_{2} < H e < C O_{2} (I I) O_{2} > C H_{4} > H_{2}

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(I) H e < H_{2} < C O_{2} < O_{2} (I I) C H_{4} > H_{2} > O_{2}

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Solution

The correct option is B $(I) H_{2} < H e < O_{2} < C O_{2} (I I) C H_{4} > O_{2} > H_{2}$
As per actual data's
sequence of Vander Wall constant (a)
$H_{2} (0.244) < H e (0.34) < O_{2} (1.36) < C O_{2} (3.54)$
and sequence of Vander Wall constant (b)
$C H_{4} (0.042) > O_{2} (0.031) > H_{2} (0.026)$

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Similar questions

Q. For real gas van der Waals equation is written as:

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

Where

a

and

b

are van der Waals constants.

Two sets of gases are:

(I) O_{2}, {C O}_{2}, H_{2}

and

H e

(I I) {C H}_{4}, O_{2}

and

H_{2}

The gases given in set-I in increasing order of

^{'} b^{'}

and gases given in set-II in decreasing order of

^{'} a^{'}

are arranged below. Select the correct order from the following:

Q. For real gases van der Waals' equation is written as

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

where a and b are van der Waals' constants. Two sets of gases are
(I)

O_{2}, C O_{2}, H_{2} and H e

(II)

C H_{4}, O_{2} and H_{2}

The gases given in set-I in increasing order of b and gases given in set - II in decreasing order of a, are arranged below. Select the correct order from the following:

Q. 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

For real gases the relation between, P, V and T is given by van der Waals' equation

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

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.

(i) Arrange the following gases in the increasing order of 'b' Give reason.

$O_{2}, C O_{2}, H_{2}, H e$

(ii) Arrange the following gases in the descending order of magnitude of 'a'. Give reason.

$C H_{4}, O_{2}, H_{2}$

Q. Given van der Waals constant for

N H_{3}, H_{2}, O_{2}

and

C O_{2}

are respectively

4.17, 0.244, 1.36

and

3.59

, which one of the following gases is most easily liquefied?

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The correct option is B (I)H2<He<O2<CO2(II)CH4>O2>H2As per actual data's sequence of Vander Wall constant (a) H2(0.244)<He(0.34)<O2(1.36)<CO2(3.54)and sequence of Vander Wall constant (b) CH4(0.042)>O2(0.031)>H2(0.026)

The correct option is B $(I) H_{2} < H e < O_{2} < C O_{2} (I I) C H_{4} > O_{2} > H_{2}$
As per actual data's
sequence of Vander Wall constant (a)
$H_{2} (0.244) < H e (0.34) < O_{2} (1.36) < C O_{2} (3.54)$
and sequence of Vander Wall constant (b)
$C H_{4} (0.042) > O_{2} (0.031) > H_{2} (0.026)$