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Standard XII

Chemistry

Characteristics of Chemical Equilibrium

The reaction ...

Question

The reaction $N_{2} + 3 H_{2} ⟺ 2 N H_{3}$ takes place at $450^{0} C$ . 1 mole of $N_{2}$ and 2 mole of $H_{2}$ are mixed in a 1 litre vessel and 1 mole of $N H_{3}$ is formed at equilibrium. Then Kc for the above reaction is ?

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Solution

The correct option is C 16
$K_{c}$ is the equilibrium constant formed by the formula for ratio of concentration of product to that of reactants.
We know that $2 α = 1$

Hence, $α = \frac{1}{2}$

$K_{c} = \frac{[N H_{3}]^{2}}{[H_{2}]^{3} \times [N_{2}]}$

$K_{c} = \frac{1 \times 1}{\frac{1}{2} \times \frac{1}{2} \times \frac{1}{2} \times \frac{1}{2}} = 16$

$K_{c}$ for above reaction = 16
Option C is correct answer

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The reaction N2+3H2⟺2NH3 takes place at 4500C. 1 mole of N2 and 2 mole of H2 are mixed in a 1 litre vessel and 1 mole of NH3 is formed at equilibrium. Then Kc for the above reaction is ?

The correct option is C 16Kc is the equilibrium constant formed by the formula for ratio of concentration of product to that of reactants.We know that 2α=1Hence, α=12Kc=[NH3]2[H2]3×[N2]Kc=1×112×12×12×12=16Kc for above reaction = 16Option C is correct answer

The reaction $N_{2} + 3 H_{2} ⟺ 2 N H_{3}$ takes place at $450^{0} C$ . 1 mole of $N_{2}$ and 2 mole of $H_{2}$ are mixed in a 1 litre vessel and 1 mole of $N H_{3}$ is formed at equilibrium. Then Kc for the above reaction is ?