a tank at is filled with of carbon monoxide gas and of chlorine pentafluoride gas. you can assume both gases behave as ideal gases under these conditions. calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. be sure your answers have the correct number of significant digits. carbon monoxide mole fraction: partial pressure: chlorine pentafluoride mole fraction: partial pressure: total pressure in tank:

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15-12-2022
Chemistry

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a tank at is filled with of carbon monoxide gas and of chlorine pentafluoride gas. you can assume both gases behave as ideal gases under these conditions. calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. be sure your answers have the correct number of significant digits. carbon monoxide mole fraction: partial pressure: chlorine pentafluoride mole fraction: partial pressure: total pressure in tank:

Answer :

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contexto1212 contexto1212 · Answer 1 · 2022-12-21T20:22:58-05:00

Mole fraction and Partial pressure can be calculated from the expression of mole and Ideal gas law.

Ideal gases are defined as the theoretical gasses that can be used to model the behavior of real gasses. In order for it to be considered ideal, individual gaseous particles must both not attract or repel one another and also not have any volume. The expression for ideal gas law is,

PV = n RT

Take an example, if a 6.000L tank at 19.2°C is filled with 18.0g of carbon monoxide gas and 10.6g of chlorine pentafluoride gas.

mole CO = 18/28 = 0.6428

mole ClF5 = 10.6/130.445 = 0.081260

then

mole total = 0.081260+0.6428 = 0.72406 mole

PV = n RT

P = n RT/V = (0.72406) (0.082) (19.2+273) / (6) = 2.89146 atm.

mole fraction CO = 0.6428 /0.72406 = 0.8877

Partial pressure of CO = 0.8877 *2.89146 = 2.5667 atm.

mole fraction CF5 = 1-0.8877 = 0.1123

Partial pressure of CF5 = 0.1123*2.89146 = 0.32471 atm.

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