Multiple choice

A $200\ mL$ flask contains oxygen at $200$ trim $Hg$ and a $ 300\ mL$ flask contains neon at $100$ $mm :Hg$. The two flasks are connected so that each gas fills their combined volumes. What is the partial pressure of neon in the final mixture? (Assuming no change in temperature).

  1. $60$ $mm \:Hg$
  2. $80$ $mm \:Hg$
  3. $100$$mm \:Hg$
  4. $150$ $mm \:Hg$
  5. $200$ $mm \:Hg$
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A Correct answer
Explanation

Neon initially occupies 300 mL at 100 mm Hg. After expansion into the combined 500 mL volume, its partial pressure is 100 × 300/500 = 60 mm Hg. The oxygen does not affect this calculation.

AI explanation

When the flasks are connected, the neon gas expands to fill the total combined volume of 200 mL + 300 mL = 500 mL. Using Boyle's law, the final partial pressure of neon is calculated as P2 = (100 mm Hg * 300 mL) / 500 mL. This yields a final partial pressure of neon equal to 60 mm Hg.

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