What is the total pressure in mm Hg of a gas mixture containing argon gas at 0.25 atm helium gas at 350 mm,Hg, and nitrogen gas at 360 torr.

Question

What is the total pressure in mm Hg of a gas mixture containing argon gas at 0.25 atm helium gas at 350 mm,Hg, and nitrogen gas at 360 torr.

Answer 1

To find the total pressure of a gas mixture, you need to add up the partial pressures of each component gas.

Given:
Partial pressure of argon gas = 0.25 atm
Partial pressure of helium gas = 350 mmHg
Partial pressure of nitrogen gas = 360 torr

First, let's convert all the pressure values to the same unit. Since we want the final answer in mmHg, we'll convert the given values to mmHg.

1 atm = 760 mmHg
1 torr = 1 mmHg

Partial pressure of argon gas = 0.25 atm * 760 mmHg/atm = 190 mmHg
Partial pressure of helium gas = 350 mmHg (no conversion needed)
Partial pressure of nitrogen gas = 360 torr = 360 mmHg

Now, add up all the partial pressures to get the total pressure:
Total pressure = Partial pressure of argon + Partial pressure of helium + Partial pressure of nitrogen
= 190 mmHg + 350 mmHg + 360 mmHg
= 900 mmHg

Therefore, the total pressure of the gas mixture is 900 mmHg.

Answer 2

Dalton's Law of Parital Pressure says that the total pressure of a system is the sum of the individual partial pressures of each gas. The only thing you need to do is to decide which unit and change the other two. I would change atm to mm and torr to mm.