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?

Answer 1

Let's represent the partial pressure of N2 as P(N2). Since the total pressure in the balloon is 850 mm Hg, we can write:

P(N2) + P(O2) + P(CO2) = 850 mm Hg

We are given that the partial pressures of O2 and CO2 are 450 mm Hg and 150 mm Hg, respectively. Plugging these values into the equation, we get:

P(N2) + 450 mm Hg + 150 mm Hg = 850 mm Hg

We can now solve for the partial pressure of N2:

P(N2) = 850 mm Hg - 450 mm Hg - 150 mm Hg = 250 mm Hg

So, the partial pressure of N2 in the final mixture is 250 mm Hg. The partial pressures of each gas in the final mixture are:

P(N2) = 250 mm Hg
P(O2) = 450 mm Hg
P(CO2) = 150 mm Hg