What is the total mmHg pressure in of a gas mixture containing argon gas at 0.25atm , helium gas at 385mmHg , and nitrogen gas at 345torr. ? sorry i didn't relize i left them out.
0.25 atm x (760mm/1 atm) = ? mm Hg Ar.
385 mm Hg He = 385 mm Hg He.
345 torr N2 = 345 mm Hg N2.
Ptotal in mm Hg = pAr + pHe + pN2 = ?
To find the total pressure in mmHg, you need to convert the units of argon gas and nitrogen gas to mmHg because helium gas is already given in mmHg.
Let's start by converting the given pressures to mmHg:
1) Argon gas pressure: 0.25 atm * 760 mmHg/atm = 190 mmHg
2) Helium gas pressure: 385 mmHg (already in mmHg)
3) Nitrogen gas pressure: 345 torr * 1 mmHg/1 torr = 345 mmHg
Now that we have all pressures in the same unit (mmHg), we can find the total pressure by simply adding them together:
Total pressure = Argon gas pressure + Helium gas pressure + Nitrogen gas pressure
= 190 mmHg + 385 mmHg + 345 mmHg
= 920 mmHg
Therefore, the total pressure of the gas mixture is 920 mmHg.