Question

What is the total pressure (in atm) inside of a vessel containing N2 exerting a partial pressure of 0.256 atm, He exerting a partial pressure of 203 mmHg, and H2 exerting a partial pressure of 39.0 kPa?

Answer 1

The total pressure inside the vessel is 0.908 atm

Step-by-step explanation:

Step 1: Data given

Partial pressure N2 = 0.256 atm

Partial pressure He = 203 mmHg = 0.267105 atm

Partial pressure H2 = 39.0 kPa = 0.3849 atm

Step 2: Calculate the total pressure

Total pressure = p(N2) + p(He) + p(H2)

Total pressure = 0.256 atm + 0.267105 atm + 0.3849 atm

Total pressure = 0.908 atm

The total pressure inside the vessel is 0.908 atm

Answer 2

Answer: Total pressure inside of a vessel is 0.908 atm

Step-by-step explanation:

According to Dalton's law, the total pressure is the sum of individual partial pressures. exerted by each gas alone.

`p_(total)=p_1+p_2+p_3`

`p_(N_2)` = partial pressure of nitrogen = 0.256 atm

`p_(He)` = partial pressure of helium = 203 mm Hg = 0.267 atm (760mmHg=1atm)

`p_(H_2)` = partial pressure of hydrogen =39.0 kPa = 0.385 atm (1kPa=0.00987 atm)

Thus
`p_(total)=p_(H_2)+p_(He)+p_(H_2)`

`p_(total)` =0.256atm+0.267atm+0.385atm =0.908atm

Thus total pressure (in atm) inside of a vessel is 0.908