A mix of O, N, and Ar has total pressure of 1.5 atm. The weights of the gases in the mix are 1.42g, 1.00g, and .50g. Calculate partial pressure of each gas; if volume of mix is 2L, what's the temp of the gas? At this temp, what's the root mean square speed of the N molecules?
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Expert's answer
2012-12-04T06:30:21-0500
Pi =xi*P xi = ni/n n(O2) = 1.42 g / 32 g/mol = 0.044 mol n(N2) = 1.00 g / 28 g/mol = 0.0357 mol n(Ar) = 50 g / 40 g/mol = 1.25 mol xi(O2) = 0.044/(0.044 + 0.0357+1.25) = 0.044/1.33 = 0.033 xi(N2) = 0.0357/1.33 = 0.027 xi (Ar) = 1.25 / 1.33 =0.94 Pi(O2) = 0.033*1.5= 0.0495 atm Pi(N2) = 0.027 * 1.5 = 0.0405 atm P (Ar) = 0.94*1.5 = 1.41 atm PV = nRT T = PV/nR T = 15450 Pa * 0.002 m3 / 1.33 mol *8.314 = 2.79 K
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