When the following reaction come to equilibrium- N2g- 2H2g- N2H4g the value of equilibrium constant is- Kc- 7-4-10-26then- the equilibrium mixture contains-

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Standard XII

Chemistry

Law of Mass Action

When the foll...

Question

When the following reaction come to equilibrium,
$N_{2} (g) + 2 H_{2} (g) \Leftrightarrow N_{2} H_{4} (g)$ the value of equilibrium constant is, $K_{c} = 7.4 \times 10^{- 26}$
then, the equilibrium mixture contains:

mostly products

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mostly reactants

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It can not be predicted

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sometimes reactants and sometimes products

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Solution

The correct option is C mostly reactants
When the value of the equilibrium constant $K_{c}$ is very low, the concentrations of products is very low and the concentrations of reactants is very high.
For the reaction $N_{2} (g) + 2 H_{2} (g) \Leftrightarrow N_{2} H_{4} (g)$ , $K_{c} = 7.4 \times 10^{- 26}$ . Since the value of $K_{c}$ is very low at equilibrium, the equilibrium mixture mostly contains reactants.

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Similar questions

Q. How can be the concentration of hydrazine,

N_{2} H_{4}

, could be increased in an equilibrium described by the equation.

N_{2} (g) + 2 H_{2} (g) ⇌ N_{2} H_{4} (g)

Δ H = 95 k J

Q. At

500

K, equilibrium constant,

K_{c}

for the following reaction is

5

\frac{1}{2} H_{2 (g)} + \frac{1}{2} I_{2 (g)} ⇌ H I_{(g)}

What would be the equilibrium constant

K_{c}

for the reaction:

2 H I_{(g)} ⇌ H_{2 (g)} + I_{2 (g)}

Q. In a vessel, two equilibrium are simultaneously established at the same temperature as follows :

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

.........(i)

N_{2} (g) + 2 H_{2} (g) ⇌ N_{2} H_{4} (g)

........(ii)

Initially the vessel contains

N_{2}

and

H_{2}

in the molar ratio of

9 : 13.

The equilibrium pressure is

7 P_{0}

, in which pressure due to ammonia is

P_{0}

and due to hydrogen is

2 P_{0}

. Find the values of equilibrium constant

(K_{P}^{'} s)

for both the reactions :

Equilibrium constant, K_c for the reaction

at 500 K is 0.061.

At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^–1 N₂, 2.0 mol L^–1 H₂ and 0.5 mol L^–1 NH₃. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

Q. Equilibrium constant,

K_{C}

for the reaction

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

500 K

0.061

At a particular time, the analysis shows that composition of the reaction mixture is

3.0 m o l L^{- 1} N_{2}, 2.0 m o l L^{- 1} H_{2}

and

0.5 m o l L^{- 1} N H_{3} .

Is the reaction at equilibirium and if not in which direction does the reaction tend to proceed to reach equilibrium?

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When the following reaction come to equilibrium,N2(g)+2H2(g)⇔N2H4(g) the value of equilibrium constant is, Kc=7.4×10−26then, the equilibrium mixture contains:

When the following reaction come to equilibrium,
$N_{2} (g) + 2 H_{2} (g) \Leftrightarrow N_{2} H_{4} (g)$ the value of equilibrium constant is, $K_{c} = 7.4 \times 10^{- 26}$
then, the equilibrium mixture contains: