You visited us 2 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

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?

[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

[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!

[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!

[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

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}

and

O_{2}

2300 K

are both

1.5 M

, what are the concentrations of

N O, N_{2}

and

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}

and

O_{2}

at 2300 K are both 1.40 M, the concentration of

N O

N_{2}

and

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

and

1.0

at equilibrium, the initial concentration of

N_{2}

and

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

. If

N_{2}

and

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}

and

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 $O_{2}$ .

Join BYJU'S Learning Program

The air pollutant NO is produced in automobile engines from the high temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300K. If the initial concentrations of N2 and O2 at 2300K are both 1.40M, what are the concentrations of NO,N2, and O2 when the reaction mixture reaches equilibrium?

The correct option is A [NO]=0.056M,[N2]=[O2]=1.37M N2(g)+O2(g)→2NO(g) 1.4 1.4at eqm 1.4-x 1.4-x 2xKc=(2x)2/(1.4−x)2=17×10−4;2x/(1.4−x)=4.12×10−22x=[NO]=0.056M[N2]=[O2]=1.37.

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
$K_{c} = (2 x)^{2} / (1.4 - x)^{2} = 17 \times 10^{- 4}; 2 x / (1.4 - x) = 4.12 \times 10^{- 2}$
$2 x = [N O] = 0.056 M$
$[N_{2}] = [O_{2}] = 1.37.$