Multiple choice

At constant temperature $200\space cm^3$ of $N_2$ at $720\space mm$ and $400\space cm^3$ of $O_2$ at $750\space mm$ pressure are put together in a one litre flask. The final pressure of the mixture is :

  1. $111\space mm$
  2. $222\space mm$
  3. $333\space mm$
  4. $444\space mm$
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D Correct answer
Explanation

Using Boyle's Law P1V1 = P2V2, the final pressure P = (P1V1 + P2V2) / V_total. P = (200 * 720 + 400 * 750) / 1000 = (144000 + 300000) / 1000 = 444000 / 1000 = 444 mm.

AI explanation

Using Boyle's law at constant temperature for each gas, the partial pressure of nitrogen becomes (720 * 200) / 1000 = 144 mm and the partial pressure of oxygen becomes (750 * 400) / 1000 = 300 mm. By Dalton's law of partial pressures, the final total pressure is the sum of these partial pressures, which is 144 + 300 = 444 mm. The final pressure of the mixture is 444 mm.

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