The equilibrium constants for the following are-N 2-3 H 2- 2 NH 3 K 1N 2- O 2- 2 NO K 2H 2-1-2 O 2- H 2 O K 3The equilibrium constant K of the reaction-2 NH 3-5-2 O 2 K - 2 NO -3 H 2 O- will beA- K 1 K 33 - K 2B- K 2 K 33 - K 1C- K 2 K 3 - K 1D- K 23 K 3 - K 1

The correct option is B K_2 K_3^3/K_1(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 ...

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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 constants of 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} ⇌ 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

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. The equilibrium constants of 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:

The following equilibria are given: $N_{2}$ +3 $H_{2}$ $⇋$ $2 N H_{3}$ $K_{1}$ ; $N_{2}$ + $O_{2}$ $⇋$ 2NO $K_{2}$ ;
$H_{2}$ + $\frac{1}{2}$ $O_{2}$ $⇋$ $H_{2} O K_{3}$ ;

The Equilibrium constant for the reaction $2 N H_{3}$ + $\frac{5}{2}$ $O_{2}$ $⇋$ 2NO + 3 $H_{2}$ O in terms of $K_{1}$ , $K_{2}$ and $K_{3}$ is:

Q. The following equilibrium are given

N_{2} + 3 H_{2} \to 2 N H_{3} - K_{1}

N_{2} + O_{2} \to 2 N O - K_{2}

H_{2} + 1 / 2 O_{2} \to H_{2} O - K_{3}

The equilibrium constant of reaction,

3 H_{2} + 5 / 2 O_{2} \to 2 N O + 3 H_{2} O

, in terms of

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

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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