Question

The mole fraction of nitrogen in air is 0.7808. calculate the partial pressure of N2 in air when the atmospheric pressure is 760 torr?

Answer 1

PN2 = XN2*Ptotal.

Answer 2

593.4

Answer 3

Please solve the question

Answer 4

I don't know

Answer 5

[AI-generated answer — Explain Bot]

To calculate the partial pressure of nitrogen (N2) in air, we can use Dalton's law of partial pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.

Step 1: Calculate the mole fraction of oxygen.
Since the mole fraction of nitrogen is known to be 0.7808, we can determine the mole fraction of oxygen by subtracting the mole fraction of nitrogen from 1 (since air is primarily composed of nitrogen and oxygen).

Mole fraction of oxygen (O2) = 1 - 0.7808 = 0.2192

Step 2: Calculate the partial pressure of nitrogen.
Given that the atmospheric pressure is 760 torr, we can calculate the partial pressure of nitrogen by multiplying the mole fraction of nitrogen by the total pressure.

Partial pressure of nitrogen (P(N2)) = Mole fraction of nitrogen (X(N2)) * Total pressure (P(total))

P(N2) = 0.7808 * 760 torr

P(N2) ≈ 593.41 torr

Therefore, the partial pressure of nitrogen (N2) in air when the atmospheric pressure is 760 torr is approximately 593.41 torr.