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Le Chatelier's Principle for Del N Equals to 0

The equilibri...

Question

The equilibrium constant for the equilibrium (at 1000 K)
$2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)$ is $K = 1.20$ . If you were to begin with 3.0 moles of $N O$ , 2.0 moles of $O_{2}$ and 7.0 moles of $N O_{2}$ , in a closed container at 1000 K, and allow the equilibrium to establish, then which of the following is correct:

A

The concentration of

N O_{2}

would go up

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B

The equilibrium constant would change to some other value besides 1.20

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C

There would be more than 3.0 moles of

N O

present

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D

The amount of

O_{2}

would decrease

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Solution

The correct option is C There would be more than 3.0 moles of $N O$ present
Reaction quotient (Q) for the given reaction with the given number of moles can be calculated as,
$Q = \frac{7^{2}}{3^{2} \times 2} = 2.72$
$\Rightarrow$ Q > K
$\Rightarrow$ Reaction will go backwards

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Similar questions

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