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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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1. A 10.0-liter flask contains 0.400 mole of H2, and 0.300 mole of N2 at 20°C. (a) What is the pressure, in atmospheres, inside the flask? (b) Calculate the mole fractions of the three gases?
Moles of Nitrogen = 0.3Moles of hydrogen = 0.4Volume = 10 LTemperature = 20 + 273 = 293 KPV = nRTPartial pressure of Nitrogen = 0.3×0.0821×208/10= 0.512atmPartial pressure of hydrogen=...
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A flask contains 2.00 moles of nitrogen and 2.00 moles of helium. How many grams of argon must be pumped into the flask in order to make the partial pressure of argon twice that of helium?
You can use the following law for solving this question: PfVf = P1V1 + P2V2 + P3V3 hellip; etc Pf is final pressure of the mixture Vf is Final volume...
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A flask contains 3.00 moles of nitrogen and 3.00 moles of neon. How many grams of argon must be pumped into the flask in order to make the partial pressure of argon twice that of neon?
The partial pressure of individual gas in the gas mixture can be expressed the following way: Pi = Ptotal *xi, Where Pi – is the partial pressure of individual gas...
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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 sample of helium occupies 535 ml at 988 torr and 25°C. If the sample is transferred to a 1.05 L flask at 25°C, what will be the gas pressure in the flask?
We know that ideal gas equation is PV = nRTWhere;T = Temperature = 25.5 oC = 25.5+273 = 298.5 KP = pressure = 988 mm Hg = 988/760 atm =...
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<ol><li>Calculate the volume of the original sample needed if you would use a 50 mL volumetric flask, a 100 mL volumetric flask, and a 250 mL volumetric flask to prepare a dilution of 1:25.</li></ol>
Ratio 1:25 means that there have to be 1+25 = 26 equal parts.1) The volume of the original sample needed if we would use a 50 mL volumetric flask is...
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Nitrogen tetroxide dissociates as follows: N2O4 --> 2NO2
If a 100ml flask contains 1.00gm of N2O4 that is 30% dissociated at 313K, what is the pressure inside the flask in atmospheres?
First we have to calculate an average molar mass of the equilibrium mixture M(N2O4/NO2) = 92 g/mol*0.7 + 46 g/mol*0.3 = 78 g/mol. Now, according to the gas state equation...
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If 1.00 g of liquid benzene (C6H6) is added to a 3.81 L flask at 25 °C (the vapor pressure benzene = 92 mm Hg at 25 °C). What is the final pressure of benzene in the flask in mm Hg?
Answer:PV = nRTP = 0.01*8.31*298 / 0.00381 = 6499.68 АТМ = 48.75 mm HgP final = 140.75 mm Hg
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