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In a container 96 gram O2 and 335 gram Neon is present. if total pressure of gaseous mixture is 25 atmosphere then what will be the partial pressure of neon?
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In a container 96 gram O2 and 335 gram Neon is present. if total press...
Partial Pressure of Neon Calculation:
1. Calculate moles of O2:
- Given: Mass of O2 = 96 g, Molar mass of O2 = 32 g/mol
- Moles of O2 = Mass/Molar mass = 96/32 = 3 moles
2. Calculate moles of Neon:
- Given: Mass of Neon = 335 g, Molar mass of Neon = 20.18 g/mol
- Moles of Neon = Mass/Molar mass = 335/20.18 ≈ 16.6 moles
3. Calculate total moles of gas:
- Total moles of gas = Moles of O2 + Moles of Neon = 3 + 16.6 = 19.6 moles
4. Calculate mole fraction of Neon:
- Mole fraction of Neon = Moles of Neon/Total moles of gas = 16.6/19.6 ≈ 0.8469
5. Calculate partial pressure of Neon:
- Given: Total pressure = 25 atm
- Partial pressure of Neon = Mole fraction of Neon x Total pressure
- Partial pressure of Neon = 0.8469 x 25 ≈ 21.1725 atm
Therefore, the partial pressure of Neon in the gaseous mixture is approximately 21.17 atm.
Community Answer
In a container 96 gram O2 and 335 gram Neon is present. if total press...
Approx..21atm
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In a container 96 gram O2 and 335 gram Neon is present. if total pressure of gaseous mixture is 25 atmosphere then what will be the partial pressure of neon?
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