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

Related BrainMass Solutions

• Physics Sample Question: Partial Pressure and Total Pressure

  Understanding partial pressure of a gas in a mixture, and how partial pressure relates to the mole fraction. One mole of nitrogen and three moles of hydrogen are injected into a container of volume 10 dm^3 at 298 K.

• 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.

• Dalton's Law of Partial Pressure

  Xi where Pi is partial pressure, Pt is total pressure and Xi is the mole fraction.

• Solubility of gas in liquid.

  Rearranging: From Roult's law we know that the partial pressure of one gas in a mixture of gases approximately equals the mole fraction of that gas times the total pressure (P).

• Partial pressure, pressure conversion, application of ideal gas equation, mole and mass calculation.

  61449 Partial pressure, pressure conversion, application of ideal gas Any number of green plants can photosynthesize glucose (C6H12O6) in the presence of carbon dioxide and water, and producing oxygen as the remaining product. 250 ml of oxygen was produced

• Partial Pressure of Reactant from Flow Rate

  variation of the partial pressure as determined by both the total pressure and the fraction of the gas component.

• Stereochemistry and Fractional Distillation

  What is the mole fraction of each component if 3.9g of benzene C6H6 is dissolved in 4.6g of toluene C7H8? 2. Assuming that this mixture is ideal, (ie. follows Raoult's Law) what is the partial vapor pressure of benezene in this mixture at 50 (C)?

• Equilibrium/pressure problem

  COCl2 (g)  CO (g) + Cl2 (g) Initially: 1 mole 0 mole 0 mole At Eqm. (1 - x) mole x mole x mole Total number of moles at equilibrium = 1 - x + x + x = 1 + x If total pressure is P, then Partial Press.:

• Polarity, bond dissociation energy of molecules

  2 / total moles = 0.1875 / 0.75 = 0.25 Mole fraction of CH)4 = moles of CH_4 / total moles = 0.5625 / 0.75 = 0.75 Partial pressure of O_2 = mole fraction of O_2 x total pressure = 0.25 x 1.12 = 0.28 atm Partial pressure of CH_4 = mole fraction