A tank holds a mixture of oxygen and nitrogen gases. If the partial pressure of oxygen is 3.3 atm and the mole fraction of N₂ gas X(N₂) = 0.78, what are the total pressure in the tank and the partial pressure of N₂?

Question

Quizplus · Accepted Answer

The total pressure in the tank is the sum of the partial pressures of the two gases:Ptotal = PO2 + PN2We are given that PO2 = 3.3 atm and X(N2) = 0.78. The mole fraction of a gas is equal to its partial pressure divided by the total pressure:X(N2) = PN2 / PtotalSolving for PN2, we get:PN2 = X(N2) * PtotalSubstituting the given values, we get:PN2 = 0.78 * PtotalNow we can substitute this expression for PN2 into the equation for Ptotal:Ptotal = PO2 + PN2Ptotal = 3.3 atm + 0.78 * Ptotal0.22 * Ptotal = 3.3 atmPtotal = 15 atmTherefore, the total pressure in the tank is 15 atm.The partial pressure of N2 is:PN2 = 0.78 * PtotalPN2 = 0.78 * 15 atmPN2 = 11.7 atmTherefore, the partial pressure of N2 is 11.7 atm.

A Tank Holds a Mixture of Oxygen and Nitrogen Gases