Chemistry High School

Atmospheric pressure at sea level is 1 bar.
A) If we climb a mountain and the pressure at the top is 0.5 bar, what is the partial pressure of oxygen? (assume at sea level the concentration of oxygen in 21\%) (1 mark)
B) If I have balloon with a volume of 1 I at sea level, what is its volume at the top of the mountain where the total pressure is 0.5 bar? (1 mark)
C) If the atmosphere on Mars is made up of an equal mix of nitrogen and carbon dioxide (50:50) and the total atmospheric pressure is 0.8 bar, what is the partial pressure of nitrogen? (1 mark)

Answers

Answer 1

A) The partial pressure of oxygen at the mountain top is 0.105 bar.

B) The balloon's volume at the mountain top is 2 I.

C) The partial pressure of nitrogen on Mars is 0.4 bar.

A) The partial pressure of a gas is calculated by multiplying the total pressure by the fraction of the gas in the mixture. In this case, the partial pressure of oxygen at the top of the mountain would be 0.5 bar multiplied by the concentration of oxygen at sea level, which is 0.21, resulting in 0.105 bar.

B) Boyle's law states that the volume of a gas is inversely proportional to its pressure at a constant temperature. Therefore, if the pressure decreases from 1 bar to 0.5 bar, the volume of the balloon would double, so its volume at the top of the mountain would be 2 I.

C) In a mixture of nitrogen and carbon dioxide with equal proportions (50:50) and a total atmospheric pressure of 0.8 bar, each gas contributes equally. Therefore, the partial pressure of nitrogen would be half of the total pressure, resulting in 0.4 bar.

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