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A mixture of 3 moles of N2, 5 moles of CO2, and 10moles of Cl2 exert a total pressure of 1120 mmHg. What is the partial pressure of CO2?

User Jhoepken
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Answer:

A mixture of 3 moles of N2, 5 moles of CO2, and 10moles of Cl2 exert a total pressure of 1120 mmHg. What is the partial pressure of CO2?

Step-by-step explanation:

According to Dalton's law of partial pressures:

The partial pressure of a gas can be determined by using the formula:


the partial pressure of a gas = mole fraction of the gas * total pressure

Partial pressure of CO2:


partial pressure of CO2= total pressure * mole fraction of CO2\\\\Mole fraction of CO2=(number of moles of CO2)/(total number of moles of all the gases) \\mole fraction of CO2=(5mol)/(3mol+5mol+10mol) = 5/18\\Partial pressure of CO2=(5)/(18) * 1120mmHg\\ =311.1mmHg

Hence, the partial pressure of CO2 is 311.1mmHg.

User Shifenis
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