Question

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?

Answer 1

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.