For the reversible reaction N2(g)+3H2(g)⇌2NH3(g) at 5000C. The value of Kp is 1.44×10−5, When partial pressure is measured in atmospheres. The corresponding value of Kc with concentration in mol L−1 is

Kp=Kc(RT)Δn Δn=2−4=−2 ⇒Kc=Kp(RT)−Δn = 1.44×10−5(0.082×773)−2

For the reversible reaction N2(g)+3H2(g)⇌2NH3(g) at 5000C. The value of Kp is 1.44×10−5, When partial pressure is measured in atmospheres. The corresponding value of Kc with concentration in mol L−1 is

Kp=Kc(RT)Δn Δn=2−4=−2 ⇒Kc=Kp(RT)−Δn = 1.44×10−5(0.082×773)−2

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For the reversible reaction $N_{2}_{(g)} + 3 H_{2}_{(g)} ⇌ 2 N H_{3}_{(g)}$ at $500^{0} C .$ The value of $K_{p}$ is $1.44 \times 10^{- 5},$ When partial pressure is measured in atmospheres. The corresponding value of $K_{c}$ with concentration in $m o l L^{- 1}$ is

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$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 500)}^{- 2}}$

$\frac{1.44 \times 10^{- 5}}{{(8.314 \times 773)}^{- 2}}$

$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 500)}^{2}}$

$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 773)}^{- 2}}$

answer is D.

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$K_{p} = K_{c} {(R T)}^{Δ n} Δ n = 2 - 4 = - 2$

$\Rightarrow K_{c} = K_{p} {(R T)}^{- Δ n}$

$= \frac{1.44 \times 10^{- 5}}{{(0.082 \times 773)}^{- 2}}$

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For the reversible reaction N2(g)+3H2(g)⇌2NH3(g) at 5000C. The value of Kp is 1.44×10−5, When partial pressure is measured in atmospheres. The corresponding value of Kc with concentration in mol L−1 is

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For the reversible reaction $N_{2}_{(g)} + 3 H_{2}_{(g)} ⇌ 2 N H_{3}_{(g)}$ at $500^{0} C .$ The value of $K_{p}$ is $1.44 \times 10^{- 5},$ When partial pressure is measured in atmospheres. The corresponding value of $K_{c}$ with concentration in $m o l L^{- 1}$ is