A mixture of He He , N 2 N2 , and Ar Ar has a pressure of 22.1 22.1 atm at 28.0 28.0 °C. If the partial pressure of He He is 2475 2475 torr and that of Ar Ar is 1049 1049 mm Hg, what is the partial pressure of N 2 N2 ?

17.47 atm

Explanation:

We need to do some conversions of units to determine this answer

Mixture of gases: He, N₂ Ar

Total pressure: 22.1 atm

Sum of partial pressures of each gas from the mixture = Total pressure

Partial pressure He + Partial pressure N₂ + Partial pressure Ar = 22.1 atm

Partial pressure N₂ = 22.1 atm - Partial pressure He - Partial pressure Ar

We convert partial pressures Ar and He to atm

2475 Torr . 1atm / 760 Torr = 3.25 atm → Partial pressure He

1049 mmHg . 1 atm / 760 mmHg = 1.38 atm → Partial pressure Ar

We replace data:

Partial Pressure N₂ = 22.1 atm - 3.25 atm - 1.38 atm → 17.47 atm

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: