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

Answer: Total pressure inside of a vessel is 0.908 atm

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

Answer 2

Answer:

The total pressure inside the vessel is 0.908 atm

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