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Mama L
4 days ago
12

A 1.00 l sample of a gas at 25.0◦c and 1.00 atm contains 50.0 % helium and 50.0 % neon by mass. what is the partial pressure of

the neon. express your answer in atmospheres.
Physics
2 answers:
kicyunya [2.9K]4 days ago
8 0
The neon's partial pressure amounts to 0.16 atm. Explanation: A 1.00 L gas sample at 25.0°C and 1.00 atm has 50.0 % helium and 50.0 % neon by mass. The partial pressure represents what the pressure of a single gas would be if it occupied the whole volume alone at the same temperature. Given the 50.0 % helium and 50.0 % neon by mass, we utilize the ideal gas equation to determine the moles and mass of the gases involved. The molar volume is defined as the volume occupied by one mole of a gas under specified temperature and pressure.
inna [2.7K]4 days ago
5 0
V = Volume of gas sample = 1.00 L = 0.001 m³T = temperature of gas = 25.0 °C = 25 + 273 = 298 K P = pressure = 1.00 atm = 101325 Pa n = number of moles of gas using ideal gas law:PV = n RT101325 (0.001) = n (8.314) (298)n = 0.041 n₁ = moles of heliumn₂ = moles of neonm₁ = mass of helium = n₁ (4) = 4 n₁m₂ = mass of neon = n₂ (20.2) = 20.2 n₂given that:m₁ = m₂4 n₁ = 20.2 n₂n₁ = 5.05 n₂also n₁ + n₂ = n5.05 n₂ + n₂ = 0.041n₂ = 0.0068mole fraction of neon is mole fraction = n₂ /n = 0.0068/0.041 = 0.166P₂ = partial pressure of neon =(mole fraction) P P₂ = (0.166) (1)P₂ = 0.166 atm
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