For the reversible reaction,N2(g)+3H2(g)⇌2NH3(g) at 500°C, the value of Kp is 1.44×10-5, when the partial pressure is measured in atmospheres. The corresponding value of KC with concentration in molL-1 is

# For the reversible reaction,${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)⇌2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$when the partial pressure is measured in atmospheres. The corresponding value of ${\mathrm{K}}_{\mathrm{C}}$ with concentration in ${\mathrm{molL}}^{-1}$ is

1. A

$1.44×{10}^{-5}/\left(0.082×500{\right)}^{-2}$

2. B

$1.44×{10}^{-5}/\left(8.314×773{\right)}^{-2}$

3. C

$1.44×{10}^{-5}/\left(0.082×773{\right)}^{2}$

4. D

$1.44×{10}^{-5}/\left(0.082×773{\right)}^{-2}$

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### Solution:

T=273+500=773

${\mathrm{K}}_{\mathrm{C}}=\frac{{\mathrm{K}}_{\mathrm{p}}}{{\left({\mathrm{RT}}^{\text{'}}\right)}^{\mathrm{\Delta n}}}=\frac{1.44×{10}^{-5}}{\left(0.082×773{\right)}^{-2}}$

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