The equilibrium constants for the following are- N2-3H2- 2NH3 K1N2-O2 - 2NO K2H2-1-2 O2 - H2O K3The equilibrium constant K of the reaction-2NH3-5-2 O2 K- 2NO-3H2 O- will be

(I) N_2+3H_2 ⇌ 2NH_3;K_1 = [NH_3]^2/[N_2][H_2]^3 (II) N_2+O_2 ⇌ 2NO; K_2 = [NO]^2/[N_2][O_2] (III) H_2+ 1/2 O_2 ⟶ H_2O;K_3 = [H_2O]/[O_2]^1/2 (II + 3 × III – ...

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Byju's Answer

Standard XII

Chemistry

Effective Equilibrium Constant

The equilibri...

Question

The equilibrium constants for the following are:
$N_{2} + 3 H_{2} ⇌ 2 N H_{3} K_{1}$
$N_{2} + O_{2} ⇌ 2 N O K_{2}$
$H_{2} + \frac{1}{2} O_{2} \to H_{2} O K_{3}$
The equilibrium constant (K) of the reaction:
$2 N H_{3} + \frac{5}{2} O_{2} K ⇌ 2 N O + 3 H_{2} O,$ will be

K_{1} K_{3}^{3} / K_{2}

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K_{2} K_{3}^{3} / K_{1}

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

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K_{2}^{3} K_{3} / K_{1}

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Solution

The correct option is B $K_{2} K_{3}^{3} / K_{1}$
$(I) N_{2} + 3 H_{2} ⇌ 2 N H_{3}; K_{1} = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}} (I I) N_{2} + O_{2} ⇌ 2 N O; K_{2} = \frac{[N O]^{2}}{[N_{2}] [O_{2}]} (I I I) H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O; K_{3} = \frac{[H_{2} O]}{[O_{2}]^{\frac{1}{2}}}$
$(I I + 3 \times I I I - I I)$ will give
$2 N H_{3} + \frac{5}{2} O_{2} K ⇌ 2 N O + 3 H_{2} O$
$∴ K = K_{2} \times K_{3}^{3} / K_{1}$

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Similar questions

Q. The equilibrium constant of the following are:

N_{2} + 3 H_{2} ⇌ 2 N H_{3}; K_{3}

N_{2} + O_{2} ⇌ 2 N O; K_{2}

H_{2} + \frac{1}{2} O_{2} ⇌ H_{2} O; K_{1}

The equilibrium constant (K) for the reaction,

2 N H_{3} + 5 / 2 O_{2} K ⇌ 2 N O + 3 H_{2} O

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}

Calculate 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)

Q. The following equilibrium constants are given

N_{2} + 3 H_{2} ⇌ 2 N H_{3}; K_{1}

N_{2} + O_{2} ⇌ 2 N O; K_{2}

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

The equilibrium constant for the oxidation of the

N H_{3}

by oxygen to give

N O

is:

The following equilibrium constants are given

$N_{2} + 3 H_{2} ⇌ 2 N H_{3}; K_{1}$

$N_{2} + O_{2} ⇌ 2 N O; K_{2}$

$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O; K_{3}$

The equilibrium constant for the oxidation of $N H_{3}$ by oxygen to give $N O$ is:

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The equilibrium constants for the following are: N2+3H2⇌2NH3 K1 N2+O2⇌2NO K2 H2+12O2→H2O K3 The equilibrium constant (K) of the reaction: 2NH3+52O2K⇌2NO+3H2O, will be

The correct option is B K2K33/K1(I)N2+3H2⇌2NH3;K1=[NH3]2[N2][H2]3(II)N2+O2⇌2NO;K2=[NO]2[N2][O2](III)H2+12O2⟶H2O;K3=[H2O][O2]12 (II+3×III–II) will give 2NH3+52O2K⇌2NO+3H2O ∴ K=K2×K33/K1

The equilibrium constants for the following are:
$N_{2} + 3 H_{2} ⇌ 2 N H_{3} K_{1}$
$N_{2} + O_{2} ⇌ 2 N O K_{2}$
$H_{2} + \frac{1}{2} O_{2} \to H_{2} O K_{3}$
The equilibrium constant (K) of the reaction:
$2 N H_{3} + \frac{5}{2} O_{2} K ⇌ 2 N O + 3 H_{2} O,$ will be