Nitrogen gas was injected into an equilibrium mixture of $2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)$ , the pressure is increased from $1.0 a t m to 10 a t m$ . Which of the following statements is correct?

The concentration of the reacting gases are unchanged.

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[S O_{2}]

increases

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[S O_{3}]

increases

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[O_{2}]

increases

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Solution

The correct option is A The concentration of the reacting gases are unchanged.
Analysing the equilibrium:

$2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)$

Nitrogen gas does not react with the given reaction mixture. The pressure increases, but since the volume remains the same, the partial pressures of all the reacting gases remain unaltered. Thus, the concentration of the reacting gases are unchanged.
So, option (A) is the correct answer.

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Similar questions

Q. To an equilibrium mixture of

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

some helium, an inert gas, is added at constant volume. The addition of helium causes the total pressure to double. Which of the following is true?

Q. The equilibrium constant

K_{p}

of the reaction:

2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)

is 900 atm at 800 K. A mixture containing

S O_{3}

and

O_{2}

having initial partial pressure of 1 and 2 atm. respectively is heated at constant volume to equilibriate. Calculate the partial pressure of

O_{2}

gas at 800 K.

The equilibrium constant Kp of the reaction, 2 $S O_{2}$ (g) + $O_{2}$ (g) $\leftrightharpoons$ 2 $S O_{3}$ (g) is 900 atm. at 800 K. A mixture containing $S O_{3}$ and $O_{2}$ having initial pressure of 1 and 2 atm respectively is heated at constant volume to equilibrate. Calculate the partial pressure of $S O_{2}$ gas at 800 K.