Question

Suppose that Daniel has a 2.50 L bottle that contains a mixture of O, N, and CO, under a total pressure of 6.00 atm. He knows that the mixture contains 0.23 mol N, and that the partial pressure of Co, is 0.250 atm. If the temperature is 273 K. what is the partial pressure of O,?

Answer 1

Dear student,

We have 2019/10/30 22:30 given volume 8= 2.50L Total pressure 8= 6:00 alm of Oz Na and CO2- Moles of Na= 0: 23 moles Partial faceasure of Co2 = 0. 250 alm Temperature = 2736 from ideal gas law PV = nRT h= PV = 6.00% 2.5 - RT 0.08206 x 273 n= 15 n = 0.667mol. Now . So farom Callan's laws of Patial fresume Piz kix Ptotal P; - the partial pressure of componenti

Ki= make fraction in the mixture Ptotal- tobal pressure of the mixture 2019/10/30 22:31 { xi = number of moles ofi tatal number of moles P (Na) = Protal X Kova Kona = 0.23 0.669 7 0.348 moles P (N2) = 6.00 x 0.348 = 2.088 atm Ptotal = P(Na) + Plow) + P (CO2) 6.00 = 2088 +Poa) + 0.250 atm Pro) 6.00 – 2.338 [ Proa) = 3:662 alm

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