CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Dalton's Law of Partial Pressures

The equilibri...

Question

The equilibrium constant , $K_{p}$ for the reaction $2 S O_{2} (g)$ $⇌$ $2 S O_{3} (g) i s 4.0 a t m^{- 1}$ at $1000 K$ . What would be the partial pressure of $O_{2}$ at the equilibrium.

A

16.0 a t m

No worries! We‘ve got your back. Try BYJU‘S free classes today!

B

0.25 a t m

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

C

1 a t m

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

0.75 a t m

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $0.25 a t m$
$2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$
$K_{p} = \frac{P^{2} S O_{3}}{P^{2} S O_{2} . P O_{2}}$
Given data $K_{p} = 4 a t o m^{- 1}$
$[S O_{2}] = [S O_{3}]$
$P S O_{2} = P S O_{3}$
$4 = \frac{1}{P O_{2}}$
$P O_{2} = 0.25 a t m$

Suggest Corrections

thumbs-up

0

Similar questions

Q. The equilibrium constant

K_{p}

for the reaction

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

1000 K

is 3.5. What would be the partial pressure of

O_{2}

gas with equal moles of

S O_{2}

S O_{3}

at equilibrium?

Q. A sample of pure

N O_{2}

1000 K

2 N O_{2} (g) ⇌ 2 N O (g) + O_{2} (g)

. The equilibrium constant

K_{P}

100 a t m

. Analysis shows that the partial pressure of

O_{2}

0.25 a t m

at equilibrium. The partial pressure of

N O_{2}

at equilibrium is:

Q. The equilibrium constant

K_{p}

for the reaction,

N_{2} (g) + O_{2} (g) ⇋ 2 N O (g)

1500^{o} C

120

N_{2}

O_{2}

at an initial pressure of

0.25 a t m

each are maintained at

1500^{o} C

till equilibrium is established, calculate the partial pressure of

N_{2}, O_{2}

N O

in the equilibrium mixture.

Q. The value of

K_{p}

for the reaction,

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

5

.
What will be the partial pressure of

O_{2}

at equilibrium when equal moles of

S O_{2}

S O_{2}

are present at equilibrium?

Q. The equilibrium constant

K_{p}

for the reaction,

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

900 {a t m}^{- 1}

800 K

. A mixture containing

{S O}_{3}

O_{2}

having initial partial pressure of

1

2 a t m

respectively is heated at constant volume to equilibriate. Calculate the partial pressure of each gas at

800 K

at equilibrium.

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Dalton's Law of Partial Pressure

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Dalton's Law of Partial Pressures

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon