total pressure of the helium and oxygen mixture

Related BrainMass Solutions

• Component Mass in Final State

  According to the Law of Partial Pressures, Moles of N2 = 0.79*1.146 = 0.90534 Moles of O2 = 0.21*1.146 = 0.24066 Now, when Helium is introduced, the partial pressures of the gases when the total pressure is 136 kPa, the calculations are given below

• moles percentage of helium-oxygen mixture

  208265 Mole percent of Helium-Oxygen Mixture I am trying to figure out what percent (by moles) of He is present in a helium-oxygen mixture having a density of 0.528g/L at 25C and 721mmHg (torr).

• Partial pressure, mole fraction, total pressure and pressure conversion.

  61461 Partial pressure, mole fraction, total pressure and pressure conversion. A tank contains 3.0 moles of nitrogen, 2.0 moles of oxygen, 1.5 moles of helium, and 1.8 moles of carbon dioxide at 45C and under 1000 atm.

• Dalton's Law of Partial Pressure

  9682 Dalton's Law of Partial Pressure A mixture of helium and neon gases is collected over water at 28.0 C and 745 mmHg. if the partial pressure of helium is 368 mmHg, what is the partial pressure of neon?

• Constant-Pressure Conditions of Hydrogen Gas

  A 2.5L flask at 15 degreesC contains a mixture of three gases, N2, He, and Ne, at partial pressures of N2-0.32 atm, He-0.15 atm, Ne-0.42 atm. a) Calculate the total pressure of the mixture.

• Pressure of Oxygen Mixtures

  39378 Pressure of Oxygen Mixtures How can i find the pressure of oxygen if it's in a mixture of .40 moles of oxygen and .20 moles of nitrogen at 1.2 atm pressure Partial pressure of O2 = (moles of Oxygen/Total number of moles)*Total pressure = (0.4/

• Partial pressure

  R= Gas constant= 0.082058 L.atm.mol ^-1K ^-1 Therefore P=Pressure= 0.0142140 atm =(0.25*0.082058*277.15)/400 Thus the calculation of pressure of Helium is correct In a mixture of two gases the total

• Determining the initial mole and mass fractions of oxygen and nitrogen in a mixture using Dalton's law of partial pressure. Solution in MS Word.

  According to Dalton's law of partial pressures we have: p(O2) = x(O2)*p where p(O2) is partial pressure of O2 in the mixture, x(O2) is mole fraction of oxygen in the mixture and p is total pressure of mixture.

• Determining the Atmospheric Pressure of Partial Pressures

  So the question comes down to, how does one determine the total pressure of a mixture of gases?