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A mixture of two gases with a total pressure of 2.00 atm contains 0.70 atm of Gas A. What is the partial pressure of Gas B in atm?
(2-0.7)=atm1.3atm
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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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At 25°C, the vapor pressure of benzene, C6H6, is 95 torr, snd toluene, C7H8, is 28 torr. Find the total pressure of the solution containing 30% C6H6 and 70% C7H8.
30% of 95torr = 28.570% of 28 torr= 19.6Total pressure = 28.5+19.6= 48.1 torr
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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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A mixture of 90.0 grams of CH4 and 10.0 grams of argon has a pressure of 250 torr under conditions of constant temperature and volume. The partial pressure of CH4 in torr is:
Molar mass of CH4 = 16.04 g/molMolar mass of argon = 39.9g/molFrom the given masses we can calculate number of moles followed by mole fraction of each gas.Number of moles...
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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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What is the partial pressure of sulfur dioxide gas in torr in a sealed vessel that has a total pressure of 520 torr and partial pressures of 0.35 atm for nitrogen?
P_gen=P(〖SO〗_2 )+P(N_2) P(〖SO〗_2 )= P_gen-P(N_2) 1 atm = 760 torr P(N_2 )=(760 torr×0.35 atm)/(1 atm)=266 torr P(〖SO〗_2 )= 520-266=254 (torr) Answer: 254 torr.
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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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