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
Answer:
-utilize precisely the same apparatus
-maintain identical measures (release height)
Explanation: