Two gases A and B having molar mass 60 and 45 , respectively, are enclosed in a vessel. The mass of A is 0 . 50 g and that of B 0 . 2 g . The total pressure of the mixture is 750 mm Hg . Calculate partial pressure of the two gases.

∵ Moles n = W mass M molar mass For gas ‘ A ’ , n A = W A M A = 0 . 5 60 moles For gas ‘ B ’ , n B = W B M B = 0 . 2 45 moles Given total pressure P T = 750 mm of Hg According to Dalton's law, Partial pressure P = Total pressure P T × Mole fraction X P A = X A · P T P A = n A n A + n B × P T P A = 0 . 5 60 0 . 5 60 + 0 . 2 45 × 750 P A = 489 . 23 mm of Hg P B = X B · P T P B = n B n A + n B × P T P B = 0 . 2 45 0 . 5 60 + 0 . 2 45 × 750 P B = 260 . 77 mm of Hg

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Which of the following graphs show the behaviour of an ideal gas?

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Important Questions on States of Matter

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.2>Q 13

The temperature of an ideal gas can be increased by

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 1

Calculate the total pressure in a

10

litre cylinder which contains

0.4 g

of helium,

1.6 g

of oxygen and

1.4 g

of nitrogen at

27 ° C

. Also calculate the partial pressure of helium gas in the cylinder. Assume ideal behavior of gases. Given,

R = 0.082 litre - atm K^{- 1} {mol}^{- 1}

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 2

Equal masses of ${CH}_{4}$ and $O_{2}$ are mixed in an empty container of one litre at $27 ° C$ . Calculate the

(a) fraction of total pressure exerted by $2 g$ of the mixture.

(b) total pressure, if the masses of gases are $32 g$ each.

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 3

Two gases

A

and

B

having molar mass

60

and

45

, respectively, are enclosed in a vessel. The mass of

A

0.50 g

and that of

B 0.2 g

. The total pressure of the mixture is

750 mm Hg

. Calculate partial pressure of the two gases.

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 4

Pure

O_{2}

diffuses through an aperture in

224 s

, whereas mixture of

O_{2}

and another gas containing

80 %

O_{2}

diffuses from the same is

234 \sec

. What is the molar mass of the gas?

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JEE Main

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 5

A mixture containing

1.12 L

D_{2}

and

2.24 L

H_{2}

NTP

is taken inside a bulb connected to another bulb through a stop cock with a small opening. The second bulb is fully evacuated. The stopcock is opened for a certain time and then closed. The first bulb is now found to contain

0.10 gm

D_{2}

. Determine the

%

by mass of the gases in second bulb.

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 6

Three grams of helium diffuses from a container in

15 \min

. The mass of sulphur dioxide diffusing from the same container over the same time interval will be

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 4 - States of Matter>DPP 4.3>Q 7

5 s

, the volume

X

H_{2}

gas effuses through a hole in a container. The time taken for the effusion of the same volume of the specified gas under identical conditions is

Which of the following graphs show the behaviour of an ideal gas?

Important Questions on States of Matter

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