Partial Pressures and Mole Fractions

Partial Pressures and Mole Fractions - a) A synthetic...

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Partial Pressures and Mole Fractions The ratio of the partial pressure of one component of a gas to the total pressure is: thus. .. The value (n 1 /n t ) is termed the mole fraction of the component gas The mole fraction ( X ) of a component gas is a dimensionless number, which expresses the ratio of the number of moles of one component to the total number of moles of gas in the sample The ratio of the partial pressure to the total pressure is equal to the mole fraction of the component gas The above equation can be rearranged to give: The partial pressure of a gas is equal to its mole fraction times the total pressure Example
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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.

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