For the chemical equilibrium - 2NOg-O2g- 2NO2gKP-1-3- 10-2 at 1000 K- What is the value of KC at 1000 K-

K_P=K_C(RT)^Δ n 1.3× 10^ 2=K_C× (0.0821× 1000)^ 1 K_C=1.3× 10^ 2× 82.1=1.067 ...

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Standard XII

Chemistry

Thermodynamic Processes

For the chemi...

Question

For the chemical equilibrium : $2 N O_{(g)} + O_{2 (g)} ⇌ 2 N O_{2 (g)}$
$K_{P} = 1.3 \times 10^{- 2}$ at $1000 K$ . What is the value of $K_{C}$ at $1000 K$ ?

0.067

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5.067

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1.067

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3.067

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Solution

The correct option is C $1.067$
$K_{P} = K_{C} (R T)^{Δ n}$
$1.3 \times 10^{- 2} = K_{C} \times (0.0821 \times 1000)^{- 1}$
$K_{C} = 1.3 \times 10^{- 2} \times 82.1 = 1.067$

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For the chemical equilibrium : 2NO(g)+O2(g)⇌2NO2(g) KP=1.3×10−2 at 1000 K. What is the value of KC at 1000 K?

The correct option is C 1.067KP=KC(RT)Δn 1.3×10−2=KC×(0.0821×1000)−1 KC=1.3×10−2×82.1=1.067

For the chemical equilibrium : $2 N O_{(g)} + O_{2 (g)} ⇌ 2 N O_{2 (g)}$
$K_{P} = 1.3 \times 10^{- 2}$ at $1000 K$ . What is the value of $K_{C}$ at $1000 K$ ?

The correct option is C $1.067$
$K_{P} = K_{C} (R T)^{Δ n}$
$1.3 \times 10^{- 2} = K_{C} \times (0.0821 \times 1000)^{- 1}$
$K_{C} = 1.3 \times 10^{- 2} \times 82.1 = 1.067$