The $K_{c}$ for the given reaction will be:
$A_{2} (g) + 2 B (g) ⇌ C (g) + 2 D (s)$

K = \frac{[C] {[D]}^{2}}{[A_{2}] [B]^{2}}

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K = \frac{[C]}{[A_{2}] [B]^{2}}

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K = \frac{[A_{2}] [{B]}^{2}}{[C] [D]^{2}}

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K = \frac{[A_{2}] [{B]}^{2}}{[C]}

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Solution

The correct option is B $K = \frac{[C]}{[A_{2}] [B]^{2}}$
$A_{2 (g)} + 2 B_{(g)} ⇌ C_{(g)} + 2 D_{(g)}$
$K = \frac{[C]}{[A_{2}] [B]^{2}}$
Component of D is not considered in K because it's a solid.

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Similar questions

A reaction : $A_{2} + B \to$ Products, involves the following mechanism :
$A_{2} ⇌ 2 A (f a s t)$ (A being the intermediate)
$A + B \to k_{2} (s l o w)$ .The rate law consistent to this mechanism is :

Q. If

a, b, c

are three complex numbers such that

a^{2} + b^{2} + c^{2} = 0

and

∣ ∣ ∣ ∣ ∣ \begin{matrix} (b^{2} + c^{2}) & a b & a c a b & (c^{2} + a^{2}) & b c a c & b c & (a^{2} + b^{2}) \end{matrix} ∣ ∣ ∣ ∣ ∣ = K a^{2} b^{2} c^{2}

then

K

is -

Q. Mark the correct alternative in each of the following:

In any ∆ABC, the value of

2 a c \sin (\frac{A - B + C}{2})

is

(a)

a^{2} + b^{2} - c^{2}

(b)

c^{2} + a^{2} - b^{2}

(c)

b^{2} - c^{2} - a^{2}

(d)

c^{2} - a^{2} - b^{2}

Q. For the hypothetical reaction, the equilibrium constant (k) values are given

A \to B (k = k_{1}) B \to C (k = k_{2}) C \to D (k = k_{3})

What is the value of equilibrium constant for

A \to D

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The Kc for the given reaction will be:A2(g)+2B(g)⇌C(g)+2D(s)

The correct option is B K=[C][A2][B]2A2(g)+2B(g)⇌C(g)+2D(g)K=[C][A2][B]2Component of D is not considered in K because it's a solid.

The $K_{c}$ for the given reaction will be:
$A_{2} (g) + 2 B (g) ⇌ C (g) + 2 D (s)$

The correct option is B $K = \frac{[C]}{[A_{2}] [B]^{2}}$
$A_{2 (g)} + 2 B_{(g)} ⇌ C_{(g)} + 2 D_{(g)}$
$K = \frac{[C]}{[A_{2}] [B]^{2}}$
Component of D is not considered in K because it's a solid.