In which of the following reactions, $K_{p}$ is less than $K_{C}$ ?

N_{2} O_{4 (g)} ⇌ 2 N O_{2 (g)}

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2 H I_{(g)} ⇌ H_{2 (g)} + I_{2 (g)}

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2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}

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N_{2 (g)} + O_{2 (g)} ⇌ 2 N O_{(g)}

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Solution

The correct option is C $2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$
$K_{p}$ is less than $K_{C}$ for $2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}$ .
$Δ n = number of moles of gaseous products - number of moles of gaseous reactants$
$Δ n = 2 - (2 + 1)$
$Δ n = - 1$
$K_{p} = K_{c} (R T)^{Δ n}$
$K_{p} = K_{c} (R T)^{- 1}$
$K_{p} = \frac{K_{c}}{R T}$
$R T > 1$
$\frac{1}{R T} < 1$
$∴ K_{p} < K_{c}$

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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}]

Δ H

Δ U

K_{p}

K_{c}

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g); K_{c} = 1.8 \times 10^{- 3}

N_{2} O_{4} ⇌ 2 N O_{2} (g); K_{c} = 3 \times 10^{- 3}

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g); K_{c} = 1.3 \times 10^{- 4}

2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g); K_{c} = 1.3 \times 10^{- 5}

2 S O_{2 (g)} + 2 N O_{2 (g)} ⟶ 2 S O_{3 (g)} + 2 N O_{g}

2 N O_{(g)} + O_{2 (g)} ⟶ 2 N O_{2 (g)}

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