A mixture of 50gH2 and 50gHe has a total pressure of 1.5atm. What is the partial pressure of H2 gas?
Correct answer: A. 1.0 atm
- A. 1.0 atm
- B. 2.0 atm
- C. 1.5 atm
- D. 3.0 atm
Explanation
Partial Pressure = Mole Fraction x Total Pressure Find moles of hydrogen and helium; moles = mass/Mr; moles = 50/2 = 25 moles of hydrogen moles= 50/4 = 12.5 moles of helium Total moles = 12.5 + 25 = 37.5 moles Hence; Partial pressure of hydrogen = mole fraction x total pressure = 25/37.5 x 1.5 =1.0 atm (hence option A is the correct answer)
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About Ideal Gas Equation
The ideal gas equation, PV = nRT, relates pressure, volume, amount and absolute temperature when gas particles are assumed to have negligible volume and no intermolecular forces. Applications include finding molar mass, density or an unknown gas variable, with careful use of Kelvin temperature and consistent units, and comparison with real-gas behaviour.
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