Nitrogen: 0.781 oxygen: 0.209 argon: 0.010 (mole fraction)

what is the partial pressure or nitrogen (in torr) in the atmosphere when the atmospheric pressure is 765.0 torr?

The partial pressure of nitrogen is 597.5 torr

Explanation:

Step 1: Data given

Mol fraction of N = 0.781

Mol fraction of O = 0.209

Mol fraction Ar = 0.010

Atmospheric pressure = 765.0 torr

The partial pressure is given by  Pi = Xi * Pt

⇒ χ i  =  the mole fraction of gas  i  in the mixture

⇒ P total  = the total pressure of the mixture

Step 2: Calculate the partial pressure of nitrogen

P(N) = mol fraction of N * atmospheric pressure

P(N) = 0.781 * 765.0 torr = 597.5 torr

The partial pressure of nitrogen is 597.5 torr

chemical properties are the characteristic of matter which can only be observed by changing the chemical identity of a sample like flammability reactivity and toxicity.

answer: a chemical reaction

explanation:

im not wrong