Condition Pressure Volume Temperature Comment

initial 1.0 atm 22.4 L 273 K 1 mole of N2 gas fills the tank.
final 3.0 atm 22.4 L 273 K 2 moles of O2 gas have been added to the 1
mole of N2 gas in the tank.
Key Questions
7. What was the initial pressure caused by the nitrogen in the tank?
8. What amount of pressure do you think the nitrogen contributed to the final total pressure?
Explain your reasoning.
9. If the sum of the pressure due to the nitrogen and the pressure due to the oxygen must equal
the total pressure, what is the oxygen pressure in the model? Explain your reasoning.
10. What fraction of the pressure is due to oxygen?
11. What is the oxygen mole fraction in the tank?
12. What is the relationship between the oxygen pressure ratio in Key Question 10 and the
oxygen mole fraction in Key Question 11? Express this relationship in the form of an
equation.

7. What was the initial pressure caused by the nitrogen in the tank? 1 atm

8. What amount of pressure do you think the nitrogen contributed to the final total pressure? 1 atm. Dalton's Law of partial pressure
Explain your reasoning.

9. If the sum of the pressure due to the nitrogen and the pressure due to the oxygen must equal
the total pressure, what is the oxygen pressure in the model? Explain your reasoning. Ptotal = pN2 + pO2; therefore,
pO2 = 2 atm


10. What fraction of the pressure is due to oxygen? 2/3

11. What is the oxygen mole fraction in the tank? 2/3

12. What is the relationship between the oxygen pressure ratio in Key Question 10 and the
oxygen mole fraction in Key Question
I will leave 12 and 11 to you.

11?13? Express this relationship in the form of an
equation.

7. The initial pressure caused by the nitrogen in the tank was 1.0 atm.

8. To find the amount of pressure contributed by nitrogen to the final total pressure, we need to subtract the initial pressure of nitrogen from the final total pressure. Therefore, the nitrogen contributed a pressure of (3.0 atm - 1.0 atm) = 2.0 atm to the final total pressure.

9. We know that the sum of the pressure due to nitrogen and the pressure due to oxygen must equal the total pressure. Since we found in Question 8 that nitrogen contributed a pressure of 2.0 atm, we can subtract this from the total pressure of 3.0 atm to find the oxygen pressure. Therefore, the oxygen pressure in the model is (3.0 atm - 2.0 atm) = 1.0 atm. This reasoning is based on the fact that the total pressure is the sum of partial pressures of all the gases present in the system.

10. To find the fraction of the pressure due to oxygen, we need to divide the oxygen pressure by the total pressure. Therefore, the fraction of the pressure due to oxygen is (1.0 atm / 3.0 atm) = 1/3 or approximately 0.333.

11. The oxygen mole fraction can be found by dividing the moles of oxygen by the total moles of gas in the tank. Initially, there was 1 mole of nitrogen and 2 moles of oxygen added. Therefore, the total moles of gas in the tank is 3 (1 mole of nitrogen + 2 moles of oxygen). The mole fraction of oxygen is (2 moles oxygen / 3 moles total gas) = 2/3 or approximately 0.667.

12. The relationship between the oxygen pressure ratio (fraction of pressure due to oxygen) and the oxygen mole fraction can be expressed as:
Pressure due to oxygen = Total pressure * Oxygen mole fraction
or
P(Oxygen) = P(Total) * X(Oxygen)
where P(Oxygen) is the pressure due to oxygen, P(Total) is the total pressure, and X(Oxygen) is the oxygen mole fraction.

7. To find the initial pressure caused by the nitrogen in the tank, we need to look at the given conditions. In this case, the initial pressure is 1.0 atm. This is specifically stated in the condition "initial 1.0 atm." So, the initial pressure caused by the nitrogen is 1.0 atm.

8. To determine the amount of pressure contributed by the nitrogen to the final total pressure, we need to subtract the pressure caused by other gases from the final total pressure. In this case, the final total pressure is 3.0 atm, as stated in the condition "final 3.0 atm." Since the initial pressure is caused by nitrogen gas, and there is no change in its volume or temperature, we can conclude that the nitrogen gas did not contribute any additional pressure to the final total pressure. Therefore, the nitrogen pressure contribution is 0 atm.

9. According to the given condition, the sum of the pressure due to the nitrogen and the pressure due to the oxygen must equal the total pressure. So, we can express this relationship as follows:

Nitrogen pressure + Oxygen pressure = Total pressure

Given that the nitrogen pressure contribution is 0 atm (as explained in question 8), we can rewrite the equation as:

Oxygen pressure = Total pressure - Nitrogen pressure
Oxygen pressure = Total pressure - 0 atm
Oxygen pressure = Total pressure

Therefore, the oxygen pressure in the model is equal to the total pressure. In this case, the oxygen pressure is 3.0 atm, as stated in the condition "final 3.0 atm."

10. To determine the fraction of the pressure due to oxygen, we need to calculate the ratio of the oxygen pressure to the total pressure. In this case, the oxygen pressure is 3.0 atm (as explained in question 9), and the total pressure is also 3.0 atm. Therefore, the fraction of the pressure due to oxygen is:

(oxygen pressure / total pressure) = (3.0 atm / 3.0 atm) = 1

So, the fraction of the pressure due to oxygen is 1 or 100%.

11. To find the oxygen mole fraction in the tank, we need to calculate the ratio of the number of moles of oxygen to the total number of moles of gas in the tank. In this case, we have 2 moles of oxygen and a total of 3 moles of gas (1 mole of nitrogen + 2 moles of oxygen). Therefore, the oxygen mole fraction is:

(oxygen moles / total moles) = (2 moles / 3 moles)

12. The relationship between the oxygen pressure ratio (as calculated in question 10) and the oxygen mole fraction (as calculated in question 11) can be expressed using Dalton's Law of Partial Pressure. According to Dalton's Law, the pressure exerted by a gas in a mixture is directly proportional to its mole fraction. Mathematically, this relationship can be expressed as:

(oxygen pressure / total pressure) = (oxygen moles / total moles)

So, the equation is:

(oxygen pressure / total pressure) = (oxygen moles / total moles)