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What is the total pressure of a mixture containing two gases if the partial pressure of one gas is 70 torr and the partial pressure of the other gas is 30 torr?
P1 = 70 torr , P2 = 30 torrPTotal = P1 + P2 PTotal = 70 torr + 30 torr = 100 torr
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A nitrox to gas mixture for scuba diving contains oxygen gas at 50 ATM and nitrogen gas at 90 6:00 a.m. what is the total pressure in ATM of the scuba gas mixture
Dalton's law states; The total pressure exerted by a mixture of gases is equal to the sum of the pressures of each of the different gases making up the mixture,...
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The partial pressure of gas X is 340 mm Hg. The partial pressure of gas Y is 264 mm Hg. The partial pressure of gas Z is 100 torr. What is the total pressure exerted by the gases in this system?
According to Dalton's Law of Partial Pressure;Pt= Px +Py+ Pz = (340+264+100)mmHg (since 1torr=1mmHg) = 704mmHg
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The total pressure of an O₂-Ar-He gas mixture is 1893 mmHg. If the partial pressure of Ar is 1100. mmHg and the partial pressure of He is 389 mmHg, what is the partial pressure of O₂
=341mmHg
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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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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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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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