For which of the following reaction $K_{p} = K_{c}$ ?

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

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{2 N O C l}_{(g)} ⇌ {2 N O}_{(g)} + {C l}_{2 (g)}

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H_{2 (g)} + I_{2 (g)} ⇌ {2 H I}_{(g)}

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{C O}_{2 (g)} + C_{(s)} ⇌ {2 C O}_{(g)}

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Solution

The correct option is D $H_{2 (g)} + I_{2 (g)} ⇌ {2 H I}_{(g)}$
Answer:-
$K_{P} = K_{C} {(R T)}^{Δ n}$
For $K_{P} = K_{C}; {(R T)}^{Δ n} must be 1$
$F o r {(R T)}^{Δ n} = 1; Δ n must be 0$
Hence, for the reaction -
${H_{2}}_{(g)} + {I_{2}}_{(g)} ⇌ {2 H I}_{(g)}$
$Δ n = 0$
Hence, $K_{P} = K_{C}$

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Similar questions

2 H I_{(g)} ⟶ H_{2 (g)} + I_{2 (g)}

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

2 N O_{(g)} ⟶ N_{2 (g)} + O_{2 (g)}

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

K_{P} = K_{C}

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

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

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

K_{p}

K_{c}

\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}]

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