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A mixture of Helium and Neon gases is collected over water at 28 degree Celsius and 745 mm Hg. If the partial pressure of Helium is 368 mm Hg, what is the partial pressure of Neon? Please explain.
The vapor pressure at 28 Co is of 28.3 mm Hg. Based on the Dalton’s law regarding partial pressure of gas mixture the total pressure is defined as follows: P...
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A mixture of noble gases consisting of 5.50g He and 15.0g Ne was placed in a cylinder at 1atm.What is the partial pressure of Helium in the mixture?
Molar Mass of He = 4.003Molar Mass of Ne = 20.1797= 5.5/4.003 = 1.365 moles of He= 15/20.1797 = 0.743 moles of NeTotal moles = 1.365 + 0.743 = 2.108...
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If the total air pressure is 1.05 atm, the partial pressure of carbon dioxide is 0.08 atm, and the partial pressure of hydrogen sulfide is 0.05 atm, what is the partial pressure of the remaining air?
As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm
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If a balloon is filled with He, Ne, and Ar gases at a total pressure of 2.0atm, what is the partial pressure of argon if the partial pressures of helium and neon are both 0.25atm each?
According to Dalton's law of partial pressure:Ptotal = P1 + P2 + P3 ...where Ptotal - total pressure, Pn - partial pressureHere:Ptotal = PHe + PNe + PArAs a result,...
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A gas mixture contains 4.0 g of CO(g), 11.0 g of CO₂(g) and 2.0 g of CH4 (g) in a 50.0 - L vessel. Calculate the partial pressure of each gas in the mixture.
The partial pressure of each gas in a mixture is proportional to its mole fraction.n = m / MM (CO) = 28 g/molM (CO2) = 44 g/molM (CH4) = 16.04...
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A 2.0 dm³ container contains 0.15 mol of N₂ gas and 0.20 mol of O₂ gas under a total pressure of 100 kNm⁻². Calculate the partial pressure of O₂ gas in the mixture.
Solution:Calculate the mole fraction (x) of O2 gas in the mixture:x(O2) = number moles of O2 / total number moles of gasTotal number moles of gas = Moles of...
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A mixture of four gases exerts a total pressure of 860mmHg. Gas A and B each exert 220mmHg. Gas C exerts 110mmHg. What pressure is exerted by gas D?
For this task we use the Dalton’s law which says that total pressure of mixture of gases equals to the sum of partial pressures of individual gases: Ptotal=PA+PB+PC+PD Therefore PD...
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The partial pressure of Ch4(g) is 0.145 atm and that of O2(g) is 0.200 atm in a mixture of the two gases.
What is the mole fraction of each gas in the mixture?
p_i/p_total =x_i=n_i/n_total , where x_i- mole fraction. x_(〖CH〗_4 )= (0.145 atm)/((0.145+0.200) atm)×100%=42.0%; x_(O_2 )=(0.200 atm)/((0.145+0.200) atm)×100%=58.0%. Answer: x_(〖CH〗_4 )=42.0%; x_(O_2 )=58.0%.
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Helium is a valuable gas used in industry.How many miles of helium atoms are in 6.46 g of helium
(6.46 / 4) x 6.02 x 10^23 = 9.72 x 10^23
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