MyQuestionIcon

1

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

Effect on Kc

The air pollu...

Question

The air pollutant NO is produced in automobile engines from the high temperature reaction $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{c} = 1.7 \times 10^{- 3}$ at 2300K. If the initial concentrations of $N_{2}$ and $O_{2}$ at 2300K are both 1.40M, what are the concentrations of $N O, N_{2},$ and $O_{2}$ when the reaction mixture reaches equilibrium?

A

[N O] = 0.056 M, [N_{2}] = [O_{2}] = 1.37 M

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

B

[N O] = 0.045 M, [N_{2}] = 0.23 M, [O_{2}] = 1.37 M

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

C

[N O] = 0.367 M, [N_{2}] = [O_{2}] = 2.03 M

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

D

[N O] = 0.056 M, [N_{2}] = 0.57 M, [O_{2}] = 0.12 M

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

Open in App

Solution

The correct option is A $[N O] = 0.056 M, [N_{2}] = [O_{2}] = 1.37 M$
$N_{2} (g) + O_{2} (g) \to 2 N O (g)$
1.4 1.4
at eqm 1.4-x 1.4-x 2x
$K_{c} = (2 x)^{2} / (1.4 - x)^{2} = 17 \times 10^{- 4}; 2 x / (1.4 - x) = 4.12 \times 10^{- 2}$
$2 x = [N O] = 0.056 M$
$[N_{2}] = [O_{2}] = 1.37.$

Suggest Corrections

thumbs-up

0

Similar questions

Q. The air pollutant

N O

is produced in automobile engines from the high temperature reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{2} = 16

2300 K

.If the initial concentrations of

N_{2}

O_{2}

2300 K

1.5 M

, what are the concentrations of

N O, N_{2}

O_{2}

when the reaction mixture reaches equilibrium ?

Q. The air pollutant

N O

is produced in automobile engines from the high temperature reaction

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{c} = 1.7 \times 10^{3}

at 2300 K. If the initial concentrations of

N_{2}

O_{2}

at 2300 K are both 1.40 M, the concentration of

N O

N_{2}

O_{2}

when the reaction mixture reaches equilibrium is:

Q. In the reaction,

N_{2} + O_{2} ⇌ 2 N O

, the moles/litre of

N_{2}

O_{2}

and NO respectively

0.25

0.05

1.0

at equilibrium, the initial concentration of

N_{2}

O_{2}

will be respectively.

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.

A sample of air consisting of $N_{2}$ and $O_{2}$ was heated to 2500 K until the equilibrium $N_{2}$ (g) + $O_{2}$ (g) $⇌$ 2NO (g) was established with an equilibrium constant $K_{c} = 2.1 \times 10^{- 3}$ . At equilibrium, the mole $%$ of NO was 1.8. Estimate the initial composition of air in mole fractions of $N_{2}$ and $O_{2}$ .

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Equilibrium Constants

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon