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Phosphorus pentachloride dissociates as follows in a closed reaction vessel:
${PCl}_{5 (g)} ⇌ {PCl}_{3 (g)} + {Cl}_{2 (g)}$ . If total pressure at the equilibrium of the reaction mixture is $P$ and the degree of dissociation of ${PCl}_{5}$ is $x$ , the partial pressure of ${PCl}_{3}$ will be

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Important Questions on States of Matter

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

A mixture of hydrogen and oxygen contains

40 %

hydrogen by mass when the pressure is

2.2

bar. The partial pressure of hydrogen is bar.

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

Which one is not correct mathematical equation for Dalton's Law of partial pressure? Here

P =

total pressure of gaseous mixture

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The pressure of a moist gas at

27 ° C

4 atm

. The volume of the container is doubled at the same temperature. The new pressure of the moist gas is

\dots \times 10^{- 1}

atm. (Nearest integer)
(Given: The vapour pressure of water at

27 ° C

0.4 atm

)

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

Gaseous

N_{2} O_{4}

dissociates into gaseous

N O_{2}

according to the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

300 K

and

1 atm

pressure, the degree of dissociation of

N_{2} O_{4}

0.2

. If one mole of

N_{2} O_{4}

gas is contained in a vessel, then the density of the equilibrium mixture is

:

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

Equal weights of ethane and hydrogen are mixed in an empty container at

25 ° C .

The fraction of total pressure exerted by hydrogen is

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The total pressure of a mixture of non-reacting gases

X (0.6 g)

and

Y (0.45 g)

in a vessel is

740 mm

Hg

. The partial pressure of the gas

X

mm

Hg .

(Nearest Integer)
(Given : molar mass

X = 20

and

Y = 45 g {mol}^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

A gaseous mixture of

2

moles of

A

3

moles of

B

5

moles of

C

and

10

moles of

D

is contained in a vessel. Assuming that gases are ideal and the partial pressure of

C

1.5

atm, total pressure is

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The equilibrium constant

K_{c}

of the reaction,

2 A ⇌ B + C is 0 .5 at 25^{o}

and

1 atm

. The reaction will proceed in the backward direction when concentrations

[A], [B] and [C]

are, respectively -

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

Equal masses of ethane and hydrogen are mixed in an empty container at

298 K

. The fraction of total pressure exerted by hydrogen is

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The mole fraction of dioxygen in a Neon-dioxygen mixture is

0.18 .

If the total pressure of the mixture is

25

bar, the partial pressure of neon in the mixture would be

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The percentage of pyridine

(C_{5} H_{5} N)

that forms pyridinium ion

(C_{5} H_{5} N^{+} H)

in a

0.10 M

aqueous pyridine solution

(K_{b} for C_{5} H_{5} N = 1 .7 \times 10^{- 9})

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

A mixture of

N_{2}

and

Ar

gases in a cylinder contains

7 g

N_{2}

and

8 g

Ar

. If the total pressure of the mixture of the gases in the cylinder is

27

bar, the partial pressure of

N_{2}

is:
[Use atomic masses (in

g {mol}^{- 1}

N = 14, Ar = 40

]

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The equilibrium constant,

K_{c} for 3 C_{2} H_{2} (g) ⇌ C_{6} H_{6} (g)

4 L^{2} {mol}^{- 2}

. If the equilibrium concentration of benzene is

0 .5 mol L^{- 1},

that of acetylene in

mol L^{- 1}

must be

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

' $x$ ' $g$ of molecular oxygen $(O_{2})$ is mixed with $200 g$ of neon $(Ne)$ . The total pressure of the nonreactive mixture of $O_{2}$ and $Ne$ in the cylinder is $25$ bar. The partial pressure of $Ne$ is $20$ bar at the same temperature and volume. The value of ' $x$ ' is

[Given: Molar mass of $O_{2} = 32 g {mol}^{- 1}$ . Molar mass of $Ne = 20 g {mol}^{- 1}$ ]

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

The equilibrium constants for the reactions

X ⇋ 2 Y

and

Z ⇋ P + Q

are

K_{1}

and

K_{2},

respectively. If the initial concentrations and the degree of dissociation of

X

and

Z

are the same, the ratio

K_{1} / K_{2}

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

An aqueous solution contains

0.10 M H_{2} S

and

0.20 M HCl

. If the equilibrium constant for the formation of

{HS}^{-}

from

H_{2} S

1.0 \times 10^{- 7}

and that of

S^{2 -}

from

{HS}^{-}

ions is

1.2 \times 10^{- 13}

, then, the concentration of

S^{2 -}

ions in the aqueous solution is:

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

For the decomposition of the compound, represented as

{NH}_{2} {COONH}_{4} (s) ⇌ 2 {NH}_{3} (g) + {CO}_{2} (g)

the

K_{p} = 2 .9 \times 10^{- 5} {atm}^{3}

. If the reaction is started with 1 mole of the compound, the total pressure at equilibrium would be :

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

$2 {SO}_{2} (g) + O_{2} (g) \to 2 {SO}_{3} (g)$

The above reaction is carried out in a vessel starting with partial pressure $P_{{SO}_{2}} = 250 m bar$ , $P_{O_{2}} = 750 m bar$ and $P_{{SO}_{3}} = 0 bar$ . When the reaction is complete, the total pressure in the reaction vessel is _____ $m bar$ .

(Round off of the nearest integer).

HARD

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

Liquids

A

and

B

form ideal solution for all compositions of

A

and

B

25^{\circ} C

. Two such solutions with

0.25

and

0.50

mole fractions of

A

have the total vapor pressures of

0.3

and

0.4

bar, respectively. What is the vapor pressure of pure liquid

B

in bar?

EASY

Chemistry>Physical Chemistry>States of Matter>Ideal Gas Equation

A mixture of one mole each of

H_{2}

He

and

O_{2}

each are enclosed in a cylinder of volume

V

at temperature T. If the partial pressure of

H_{2}

2 atm,

the total pressure of the gases in the cylinder is:

Phosphorus pentachloride dissociates as follows in a closed reaction vessel: PCl 5 g ⇌ PCl 3 g + Cl 2 g . If total pressure at the equilibrium of the reaction mixture is P and the degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be

Important Questions on States of Matter

Learn and Prepare for any exam you want !

Phosphorus pentachloride dissociates as follows in a closed reaction vessel:
${PCl}_{5 (g)} ⇌ {PCl}_{3 (g)} + {Cl}_{2 (g)}$ . If total pressure at the equilibrium of the reaction mixture is $P$ and the degree of dissociation of ${PCl}_{5}$ is $x$ , the partial pressure of ${PCl}_{3}$ will be