The number of moles of He in the flask when A 10.0-L flask containing He, 2.00 mole of Ar, and 3.00 mole of Ne has a total pressure of 24.5 atm at 25°C. = 5 moles
Dalton's law of partial pressure: State that in a mixture of gases, the pressure exerted by each of the gases, is the same as that which it will exert when it is alone.
Applying the general equation of gas
PV = nRT....................... Equation 1
Where P = pressure of the mixture, V = Volume, n = number of moles of the mixture, R = molar gas constant, T = Temperature of the mixture
n = PV/RT................ Equation 2
From the question,
Given: P = 24.5 atm, V = 10.0 L, T = 25°C = (25+2730) = 298K,
R = 0.082 L⋅atm⋅K−1⋅mol−1
Substitute these values into equation 2
n = (24.5×10)/(0.082×298)
n = 245/24.436
n = 10.02
n ≈ 10 moles.
Total number mole of the mixture = number of mole of He + number of mole of Ar + number of mole of Ne
10 = He+2+3
He = 10-2-3
He = 5 mole.
Therefore, the number mole of He in the flask is 5 moles
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