If N2 is added to a balloon that contains O2 (partial pressure 450 mm Hg) and CO2 (partial pressure 150 mm Hg) to give a total pressure of 850 mm Hg, what is the partial pressure of each gas in the final mixture?
To determine the partial pressure of each gas in the final mixture, we can use Dalton's Law of Partial Pressure. According to this law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.
In this case, we have three gases: N2, O2, and CO2. Let's denote the partial pressure of N2 as PN2, O2 as PO2, and CO2 as PCO2.
According to the problem, the partial pressure of O2 is 450 mm Hg, and the partial pressure of CO2 is 150 mm Hg. The total pressure of the mixture is given as 850 mm Hg.
Using Dalton's Law of Partial Pressure, we can set up the equation:
PN2 + PO2 + PCO2 = Total pressure
Plugging in the known values:
PN2 + 450 mm Hg + 150 mm Hg = 850 mm Hg
Now, let's solve for PN2:
PN2 = 850 mm Hg - 450 mm Hg - 150 mm Hg
PN2 = 250 mm Hg
Therefore, the partial pressure of N2 in the final mixture is 250 mm Hg.
To summarize:
- Partial pressure of N2 (PN2) = 250 mm Hg
- Partial pressure of O2 (PO2) = 450 mm Hg
- Partial pressure of CO2 (PCO2) = 150 mm Hg