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Standard XII

Chemistry

Derivation of Kp and Kc

Determine the...

Question

Determine the equilibrium constant for the following reaction if the equilibrium concentrations of nitrogen, hydrogen, and ammonia are 1 M, 2 M, and 15 M, respectively.
$N_{2} (g) + 3 H_{2} (g) ⇋ 2 {N H}_{3} (g)$

0.035

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7.5

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380

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None of the above

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Solution

The correct option is C 28
$a A + b B \leftrightarrow c C + d D$
$K_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$
$N_{2} + 3 H_{2} \leftrightarrow 2 N H_{3}$
$K_{c} = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}}$
$K_{c} = \frac{[15]^{2}}{[1] [2]^{3}} = 28$

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Similar questions

Q. What is the value of the equilibrium constant for the following reaction if the equilibrium concentrations of nitrogen, hydrogen, and ammonia are 1 M, 2 M, and 15 M, respectively?

N_{2} (g) + 3 H_{2} (g) ⇋ 2 {N H}_{3} (g)

1 m o l e

of nitrogen and

3 m o l e s

of hydrogen are mixed in a

4 L

container. If

0.25

percent of nitrogen is converted to ammonia by the following reaction:

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

Calculate the equilibrium constant (

K_{c}

) in concentration units. What will be the value of

K

for the following equilibrium?

\frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g) ⇌ {N H}_{3} (g)

Q. The equilibrium constant for the reaction,

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

k

, then the equilibrium constant for the equilibrium

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

is:

Q. Nitrogen and hydrogen are added to a

5

litre flask under pressure. The flask was sealed and heated. The equilibrium mixture contained

19.0 g

of ammonia,

0.16 g

of hydrogen and

3.4 g

of nitrogen. Calculate the equilibrium constant,

K_{c}

of the reaction:

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

Q. Calculate the equilibrium constant

(K c)

for the formation of

N H_{3}

in the following reaction:

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

At equilibrium, the concentration of

N H_{3}, H_{2}

and

N_{2}

are

1.2 \times 10^{- 2}, 3.0 \times 10^{- 2}

and

1.5 \times 10^{- 2} M

respectively.

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Determine the equilibrium constant for the following reaction if the equilibrium concentrations of nitrogen, hydrogen, and ammonia are 1 M, 2 M, and 15 M, respectively.N2(g)+3H2(g)⇋2NH3(g)

The correct option is C 28aA+bB↔cC+dDKc=[C]c[D]d[A]a[B]bN2+3H2↔2NH3Kc=[NH3]2[N2][H2]3Kc=[15]2[1][2]3=28

Determine the equilibrium constant for the following reaction if the equilibrium concentrations of nitrogen, hydrogen, and ammonia are 1 M, 2 M, and 15 M, respectively.
$N_{2} (g) + 3 H_{2} (g) ⇋ 2 {N H}_{3} (g)$

The correct option is C 28
$a A + b B \leftrightarrow c C + d D$
$K_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$
$N_{2} + 3 H_{2} \leftrightarrow 2 N H_{3}$
$K_{c} = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}}$
$K_{c} = \frac{[15]^{2}}{[1] [2]^{3}} = 28$