Ptotal = pHe + pN2 + pAr
You know all but one unknown.
Be careful with the units. Ptotal is in atm and the gases are given in torr (and mm but 1 mm = 1 torr)
You know all but one unknown.
Be careful with the units. Ptotal is in atm and the gases are given in torr (and mm but 1 mm = 1 torr)
First, let's convert the given pressure values to a consistent unit. We can choose to convert everything to atmospheres (atm) for convenience.
Given:
Partial pressure of He = 1525 torr
Partial pressure of Ar = 2807 mmHg
Total pressure = 14.2 atm
To convert torr to atm, divide by 760:
Partial pressure of He = 1525 torr ÷ 760 torr/atm = 2.01 atm
To convert mmHg to atm, divide by 760:
Partial pressure of Ar = 2807 mmHg ÷ 760 mmHg/atm = 3.69 atm
Now, let's use Dalton's law to find the partial pressure of N2.
Total pressure = Partial pressure of He + Partial pressure of N2 + Partial pressure of Ar
14.2 atm = 2.01 atm + Partial pressure of N2 + 3.69 atm
To solve for the partial pressure of N2, rearrange the equation:
Partial pressure of N2 = Total pressure - Partial pressure of He - Partial pressure of Ar
Partial pressure of N2 = 14.2 atm - 2.01 atm - 3.69 atm
Partial pressure of N2 = 8.5 atm
Therefore, the partial pressure of N2 in the mixture is 8.5 atm.
Step 1: Convert the partial pressures of He and Ar to atm.
To convert from torr to atm, divide the pressure by 760:
Partial pressure of He = 1525 torr / 760 torr/atm = 2.00658 atm
Partial pressure of Ar = 2807 mm Hg / 760 mm Hg/atm = 3.69145 atm
Step 2: Find the partial pressure of N2.
Total pressure of the mixture = Pressure of He + Pressure of N2 + Pressure of Ar
14.2 atm = 2.00658 atm + Pressure of N2 + 3.69145 atm
Step 3: Solve for the partial pressure of N2.
Pressure of N2 = 14.2 atm - 2.00658 atm - 3.69145 atm
Pressure of N2 = 8.50297 atm
Therefore, the partial pressure of N2 is approximately 8.5 atm.