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Standard XII

Chemistry

Characteristics of Equilibrium Constant

1 mole of N...

Question

1 mole of $N_{2}$ and 3 moles of $H_{2}$ are placed in 1L vessel. Find the concentration of ${N H}_{3}$ at equilibrium if the equilibrium constant $(K_{c})$ at 400K is $\frac{4}{27}$ .
$N_{2} (g) + {3 H}_{2} (g) ⇌ 2 N H_{3} (g)$

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Solution

Volume = 1 L
Temperature = 400 K
Equilibrium constant, $K_{c} = \frac{4}{27}$
The Net balanced chemical reaction is,
$N_{2} + 3 H_{2} \to 2 N H_{3}$
Initial concentration 1 2 0

At equilibrium (1-x) (3-3x) 2x
The expression for equilibrium constant is,

$K_{c} = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}}$
By rearranging the terms, we get the value of $x$ .

$x = 0.381 m o l e / L$
The concentration of $N H_{3}$ at equilibrium $=$ $2 x$ $= 2 \times 0.381 = 0.762 m o l e / L$

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1 mole of N2 and 3 moles of H2 are placed in 1L vessel. Find the concentration of NH3 at equilibrium if the equilibrium constant (Kc) at 400K is 427.N2(g)+3H2(g)⇌2NH3(g)

1 mole of $N_{2}$ and 3 moles of $H_{2}$ are placed in 1L vessel. Find the concentration of ${N H}_{3}$ at equilibrium if the equilibrium constant $(K_{c})$ at 400K is $\frac{4}{27}$ .
$N_{2} (g) + {3 H}_{2} (g) ⇌ 2 N H_{3} (g)$