CHY 102 Lecture Notes - Lecture 29: Mole Fraction, Ethylene, Partial Pressure
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P of a gas mixture = sum of the pressures that the components would exert individually if separated. P = p1 + p2 + p3 + + pn. For ideal gases, p1 = n1rt/v, etc. What is the p of 10. 0 g of o2 and 6. 00 g of c2h4 in a 12. 0 l bulb at 298 k? (mo2 = 32. 0 g/mol; mc2h4 = 28. 1 g/mol) Ans: no2 = (10. 0 g)/(32. 0 g/mol) = 0. 312 mol nc2h4 = (6. 00 g)/(28. 1 g/mol) = 0. 213 mol. L container at 25 c? (r=0. 083145 l bar/mol/k; 0 c = 273. 15 k: 0. 203 bar, 1. 54 bar, 2. 42 bar. What is the total pressure of a mixture of 1. 570 mol of co and 0. 870 mol no2 in a 25. 0. Partial pressure of gas a can be expressed in terms of the mole fraction of a, a: Ptotal = (pa + pb + + pn) = ntotalrt/v and.
