The decomposition reaction,
$4 H N O_{3} (g) ⇌ 4 N O_{2} (g) + 2 H_{2} O (g) + O_{2} (g)$ is started with pure $H N O_{3} (g)$ . If $p$ is the total pressure at equilibrium, then

K_{p} = \frac{(p_{O_{2}})^{7}}{(p - 7 p_{O_{2}})^{4}}

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K_{p} = \frac{1024 (p_{O_{2}})^{7}}{(p - 7 p_{O_{2}})^{4}}

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K_{p} = \frac{7 p_{O_{2}}}{(p - 4 p_{O_{2}})}

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K_{p} = \frac{(p - p_{O_{2}})^{7}}{(p - 7 p_{O_{2}})^{4}}

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Solution

The correct option is B $K_{p} = \frac{1024 (p_{O_{2}})^{7}}{(p - 7 p_{O_{2}})^{4}}$
$\begin{matrix} 4 H N O_{3} (g) & ⇌ & 4 N O_{2} (g) & + & 2 H_{2} O (g) & + & O_{2} (g) p_{0} & . . . & . . . & . . . p_{0} - 4 p_{O_{2}} & 4 p_{O_{2}} & 2 p_{O_{2}} & p_{O_{2}} \end{matrix}$
$∴ p_{0} + 3 p_{O_{2}} = p$
$∴ p_{0} = (p - 3 p_{O_{2}})$
$∴ p_{0} - 4 p_{O_{2}} = p - 3 p_{O_{2}} - 4 p_{O_{2}} = p - 7 p_{O_{2}}$
$∴ K_{p} = \frac{(4 p_{O_{2}})^{4} (2 p_{O_{2}})^{2} \times p_{O_{2}}}{(p - 7 p_{O_{2}})^{4}} = \frac{1024 \times p_{O_{2}^{2}}^{7}}{(p - 7 p_{O_{2}})^{4}}$

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Similar questions

Q. If the decomposition reaction

4 H {N O}_{2} (g) ⇌ 4 {N O}_{2} (g) + 2 H_{2} O (g) + O_{2} (g)

is started with where

(P)

is the total pressure at equilibrium and (

P^{'}

) is the partial pressure of

O_{2}

. Derive relationship for

K_{p}

is terms of (

P

) and (

P^{'}

For the decomposition reaction $4 H N O_{3} (g) ⇌ 4 N O_{2} (g) + 2 H_{2} O + O_{2}$ (g) if we start with only the reactant $H N O_{3}$ and p = equilibrium pressure, the equilibrium constant $K_{p}$ is:

For thedecomposition reaction 4 $H N O_{3}$ (g) $⇋$ 4 $N O_{2}$ (g) + 2 $H_{2}$ O (g) + $O_{2}$ (g) if we start with only the reactant $H N O_{3}$ and p = equilibrium pressure, the equilibrium constant $K_{p}$ is:

Q. For the reaction equilibrium,

2 N O B r (g) ⇋ 2 N O (g) + B r_{2} (g)

.
If

P_{B_{1}} = \frac{P}{9}

at equilibrium and

P

is total pressure, the ratio of

\frac{K_{P}}{P}

is equal to:

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The decomposition reaction, 4HNO3(g)⇌4NO2(g)+2H2O(g)+O2(g) is started with pure HNO3(g). If p is the total pressure at equilibrium, then

The correct option is B Kp=1024(pO2)7(p−7pO2)44HNO3(g)⇌4NO2(g)+2H2O(g)+O2(g)p0.........p0−4pO24pO22pO2pO2 ∴p0+3pO2=p ∴p0=(p−3pO2) ∴p0−4pO2=p−3pO2−4pO2=p−7pO2 ∴Kp=(4pO2)4(2pO2)2×pO2(p−7pO2)4=1024×p7O22(p−7pO2)4

The decomposition reaction,
$4 H N O_{3} (g) ⇌ 4 N O_{2} (g) + 2 H_{2} O (g) + O_{2} (g)$ is started with pure $H N O_{3} (g)$ . If $p$ is the total pressure at equilibrium, then