Multiple choice

The total pressure of a mixture of 6.4 grams of oxygen and 5.6 grams of nitrogen present in a 2 litre vessel is 1200 $mm$. What is the partial pressure ( in $mm$ ) of nitrogen?

  1. 1200

  2. 600

  3. 900

  4. 200
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

Moles of O2 = 6.4/32 = 0.2. Moles of N2 = 5.6/28 = 0.2. Total moles = 0.4. Partial pressure of N2 = (Moles of N2 / Total Moles) * Total Pressure = (0.2 / 0.4) * 1200 = 600 mm.

AI explanation

To find the partial pressure of nitrogen, we first determine the mole fraction of nitrogen using the ratio of its moles to the total moles in the vessel. The moles of oxygen are 6.4 divided by 32, which is 0.2, and the moles of nitrogen are 5.6 divided by 28, which is 0.2, making the mole fraction of nitrogen 0.2 divided by 0.4, or 0.5. According to Dalton's law, the partial pressure of nitrogen is its mole fraction multiplied by the total pressure, so 0.5 multiplied by 1200 mm gives 600 mm.

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