Given-N 2 g -3 H 2 g - 2 NH 3 g - K 1N 2 g - O 2 g - 2 NO g - K 2H 2 g -1-2 O 2 g - H 2 O g - K 3The equilibrium constant for 2 NH 3 g -5-2 O 2 g - 2 NO g -3 H 2 O g will be-A- K 1 K 2 K 3B- K 1 K 2- K 3C- K 2 K 33- K 1D- K 1 K 32- K 2

The correct option is C K_2K_3^3K_1K_1=[NH_3]^2[N_2[H_2]^3 K_2=[NO]^2[N_2][O_2] K_3=[H_2O][H_2][O_2]^1/2 The equilibrium constant for nbsp; 2NH_3(g)+52O_2(g) ...

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Byju's Answer

Standard XII

Chemistry

Equilibrium Constant and Standard Free Energy Change

Given:N 2 g +...

Question

Given:
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}$
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{2}$
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}$
The equilibrium constant for
$2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)$
will be:

K_{1} K_{2} K_{3}

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\frac{K_{1} K_{2}}{K_{3}}

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\frac{K_{1} K_{3}^{2}}{K_{2}}

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\frac{K_{2} K_{3}^{3}}{K_{1}}

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Solution

The correct option is D $\frac{K_{2} K_{3}^{3}}{K_{1}}$
$K_{1} = \frac{[N H_{3}]^{2}}{[N_{2} [H_{2}]^{3}}$
$K_{2} = \frac{[N O]^{2}}{[N_{2}] [O_{2}]}$
$K_{3} = \frac{[H_{2} O]}{[H_{2}] [O_{2}]^{\frac{1}{2}}}$
The equilibrium constant for
$2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)$
will be :
$\frac{[N O]^{2} [H_{2} O]^{3}}{[N H_{3}]^{2} [O_{2}]^{\frac{5}{2}}}$
$\Rightarrow \frac{K_{2} K_{3}^{3}}{K_{1}}$

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Similar questions

Q. Given:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g), K_{2}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

The equilibrium constant for,

2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

will be:

Q. Given:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

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

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

where

K_{1}, K_{2}, K_{3}

are equilibrium constants.
The equilibrium constant for the reaction,

2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

will be:

Q. Given:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

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

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

The equilibrium constant for

2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

will be:

Q. The following equilibrium constants are given:

N_{2} (g) + H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

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

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

The equilibrium constant for the oxidation of the

N H_{3}

by oxygen to give

N O

is:

2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

Q. Given:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

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

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

The equlibrium constant for the given reaction will be:

2 N H_{2} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

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Given: N2(g)+3H2(g)⇌2NH3(g);K1 N2(g)+O2(g)⇌2NO(g);K2 H2(g)+12O2(g)⇌H2O(g);K3 The equilibrium constant for 2NH3(g)+52O2(g)⇌2NO(g)+3H2O(g) will be:

The correct option is D K2K33K1K1=[NH3]2[N2[H2]3 K2=[NO]2[N2][O2] K3=[H2O][H2][O2]12 The equilibrium constant for 2NH3(g)+52O2(g)⇌2NO(g)+3H2O(g) will be : [NO]2[H2O]3[NH3]2[O2]52 ⇒K2K33K1

Given:
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}$
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{2}$
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}$
The equilibrium constant for
$2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)$
will be: