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Characteristics of Equilibrium Constant

In which of t...

Question

In which of the following equilibrium, $K_{c} = K_{p}$ ?

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

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4 N H_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (g)

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

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2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)

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Solution

The correct option is C $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$

Kp only counts with gases molecule , while Kc only counts with aqueous solution+ gases. So here reactant and product both are gaseous that's why only reaction having equal numbers of reactants and products will have kp=kc ie.change in number of moles is equal to 0.option(a) is correct.

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Similar questions

\frac{K_{p}}{K_{c}}

300 K

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

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

[A t 300 K, R T = 24.62 d m^{3} a t m m o l^{- 1}]

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); K_{1}

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g), K_{2}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (g); K_{3}

2 N H_{3} (g) + \frac{5}{2} O_{2} (g) ⇌ 2 N O (g) + 3 H_{2} O (g)

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); K_{c} = 2.7 \times 10^{- 18}

2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)

\begin{matrix} List - I & List - II (I) Dissociation of N_{2} O_{4} (g) : & (P) Increases with N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); & temperature Δ H = + 57.0 k J (II) Oxidation of N H_{3} (g) : & (Q) Decreases with 4 N H_{3} (g) + 5 O_{2} ⇌ 4 N O (g) + 6 H_{2} O (g); & pressure Δ H = - 900.0 k J (III) Oxidation of nitrogen: & (R) Increases with N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); & addition of inert Δ H = + 180.0 k J & gas at constant pressure (IV) Formation of N O_{2} (g) : & (S) Decreases with N O (g) + O_{3} (g) ⇌ N O_{2} (g) + O_{2} (g); & temperature Δ H = - 200.0 k J (T) K_{p} = K_{c} (U) K_{p} = K_{c} (R T)^{1} \end{matrix}

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

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

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