A mixture of gases contains 0.67 mol N2, 0.48 mol O2, and 0.29 mol CO2. If the total pressure of the mixture is 1.37 atm, what is the partial pressure of each component?
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0.67 + 0.48 + 0.29 = 1.44 mol
Since V and T do not change, moles are proportional to pressure
(0.67/1.44) x 1.37 atm = 0.637 atm (partial pressure of 0.67 mol N2)
(0.48/1.44) x 1.37 atm = 0.457 atm (partial pressure of 0.48 mol O2)
(0.29/1.44) x 1.37 atm = 0.276 atm (partial pressure of 0.29 mol CO2)
Since V and T do not change, moles are proportional to pressure
(0.67/1.44) x 1.37 atm = 0.637 atm (partial pressure of 0.67 mol N2)
(0.48/1.44) x 1.37 atm = 0.457 atm (partial pressure of 0.48 mol O2)
(0.29/1.44) x 1.37 atm = 0.276 atm (partial pressure of 0.29 mol CO2)