alleryStart learning →An anaesthetic mixture holds 2.83 mol oxygen and 8.41 mol nitrous oxide at a total pressure of 192 kPa. What is the partial pressure of oxygen?
A96.0 kPa
B143.6 kPa
C48.4 kPa
D24.2 kPa
Answer & Solution
Correct answer: C. 48.4 kPa
1. Partial pressure equals the mole fraction of that gas multiplied by the total pressure.
2. Total moles are 2.83 + 8.41 = 11.24 mol.
3. The mole fraction of oxygen is 2.83 / 11.24 = 0.252.
4. Multiply by the total pressure: 0.252 x 192 kPa = 48.4 kPa.
5. Oxygen is the minor component, so its partial pressure must be well under half of 192 kPa.
6. The value 143.6 kPa is the nitrous oxide share, so it is what you get by using the wrong mole fraction.
_Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions_
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