Question

Dry air is 78.08% nitrogen, 20.95% oxygen and 0.93% argon with the 0.04% being other gases. if the atmospheric pressure is 760.0 torr, what is the partial pressure of nitrogen in dry air?

Answer 1

Explanation:

Let us assume that volume of air present is 100.

So, when 78.08% nitrogen is present then it means that volume of nitrogen is 78.08.

Similarly, volume of oxygen is 20.95, volume of argon is 0.93 and volume of other gases is 0.04.

Hence, calculate the mole fraction of given gases as follows.

         Mole fraction of $N_{2}$ = $\frac{78.08}{100}$

                                               = 0.7808

         Mole fraction of $O_{2}$ = $\frac{20.95}{100}$

                                               = 0.2095

        Mole fraction of Ar = $\frac{0.93}{100}$

                                               = 0.0093

        Mole fraction of other gases = $\frac{0.04}{100}$

                                               = 0.0004

As the mole fraction of nitrogen is 0.7808 and total pressure is 760.0 torr. Therefore, calculate the partial pressure of nitrogen as follows.

                         $p_{i} = x_{i} \times P_{total}$

                                      = $0.7808 \times 760 torr$

                                       = 593.408 torr

Therefore, we can conclude that the partial pressure of nitrogen in dry air is 593.408 torr.

Answer 2

Taking  into account the Dalton's law, the partial pressure of nitrogen in dry air is 593.408 torr.

The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:

PT = PA + PB

This relationship is due to the assumption that there are no attractive forces between the gases.

Dalton's partial pressure law can also be expressed in terms of the mole fraction of the gas in the mixture. The mole fraction is a dimensionless quantity that expresses the ratio of the number of moles of a component to the number of moles of all the components present.

So in a mixture of two or more gases, the partial pressure of gas A can be expressed as:

PA = xA× PT

In this case, you know that dry air is 78.08% nitrogen, 20.95% oxygen and 0.93% argon with the 0.04% being other gases. This means that the mole fracttion are:

• Nitrogen= 0.7808
• Oxygen= 0.2095
• Argon= 0.0093
• Other gases= 0.0004

As the mole fraction of nitrogen is 0.7808 and the total pressure is 760.0 torr, the partial pressure of nitrogen can be calculated as:

Pnitrogen= 0.7808× 760 torr

Pnitrogen= 593.408 torr

Finally, the partial pressure of nitrogen in dry air is 593.408 torr.

Learn more:

• https://brainly.com/question/10737617?referrer=searchResults
• https://brainly.com/question/12740226?referrer=searchResults
• https://brainly.com/question/14623719?referrer=searchResults