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?

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

To find the partial pressure of each gas in the final mixture, we need to determine the amount of N2 added to the balloon.

Let's assume that x mm Hg of N2 is added to the balloon. Therefore, the total pressure of the mixture becomes N2 partial pressure + O2 partial pressure + CO2 partial pressure.

Given:
Partial pressure of O2 = 450 mm Hg
Partial pressure of CO2 = 150 mm Hg
Total pressure = 850 mm Hg

Using the information above, we can create the following equation:

x + 450 mm Hg + 150 mm Hg = 850 mm Hg

Simplifying the equation:

x + 600 mm Hg = 850 mm Hg

Subtracting 600 mm Hg from both sides:

x = 250 mm Hg

Therefore, 250 mm Hg of N2 is added to the balloon.

To find the partial pressure of each gas in the final mixture:
Partial pressure of N2 = 250 mm Hg
Partial pressure of O2 = 450 mm Hg
Partial pressure of CO2 = 150 mm Hg

To determine the partial pressure of each gas in the final mixture, we need to apply Dalton's Law of Partial Pressures. According to Dalton's Law, the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas.

In this case, we have a balloon containing O2, CO2, and N2. The partial pressure of O2 is given as 450 mm Hg, the partial pressure of CO2 is 150 mm Hg, and the total pressure of the mixture is 850 mm Hg.

To find the partial pressure of N2, we can use the equation:

Total pressure = Partial pressure of O2 + Partial pressure of CO2 + Partial pressure of N2

Rearranging the equation, we get:

Partial pressure of N2 = Total pressure - Partial pressure of O2 - Partial pressure of CO2

Substituting the given values, we have:

Partial pressure of N2 = 850 mm Hg - 450 mm Hg - 150 mm Hg
Partial pressure of N2 = 250 mm Hg

Therefore, the partial pressure of N2 in the final mixture is 250 mm Hg.