alleryStart learning →A 10.0 L vessel holds 2.50 x 10^-3 mol of hydrogen at 35 degrees C. What is the partial pressure of the hydrogen?
A2.53 x 10^-3 atm
B7.58 x 10^-4 atm
C9.61 x 10^-3 atm
D6.32 x 10^-3 atm
Answer & Solution
Correct answer: D. 6.32 x 10^-3 atm
1. Each gas in a mixture acts independently, so apply PV = nRT to the hydrogen alone.
2. Rearrange to P = nRT / V.
3. Convert the temperature to kelvin: 35 + 273 = 308 K.
4. Multiply moles by R: 2.50 x 10^-3 mol x 0.08206 L atm/mol K = 2.052 x 10^-4.
5. Multiply by the temperature: 2.052 x 10^-4 x 308 = 0.0632 L atm.
6. Divide by the volume: 0.0632 / 10.0 = 6.32 x 10^-3 atm.
7. The option 9.61 x 10^-3 atm is the total pressure of the whole mixture, which is the trap for anyone who adds before being asked to.
_Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions_
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