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Unformatted text preview: a) A synthetic atmosphere is created by blending 2 mol percent CO 2 , 20 mol percent O 2 and 78 mol percent N 2 . If the total pressure is 750 torr, calculate the partial pressure of the oxygen component. Mole fraction of oxygen is (20/100) = 0.2 Therefore, partial pressure of oxygen = (0.2)(750 torr) = 150 torr b) If 25 liters of this atmosphere, at 37C, have to be produced, how many moles of O 2 are needed? P O2 = 150 torr (1 atm/760 torr) = 0.197 atm V = 25 L T = (273+37K)=310K R=0.0821 L atm/mol K PV = nRT n = (PV)/(RT) = (0.197 atm * 25 L)/(0.0821 L atm/mol K * 310K) n = 0.194 mol...
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.
 Fall '10
 LauraChoudry
 Chemistry, Mole, Partial Pressure

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