1. Understand Partial Pressure

Partial pressure is the pressure exerted by a single gas in a mixture of gases. Dalton's Law of Partial Pressures states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas.

2. Calculate Mole Fractions

* Nitrogen (N2): 3 moles / (3 moles + 1 mole) = 0.75 (mole fraction)

* Hydrogen (H2): 1 mole / (3 moles + 1 mole) = 0.25 (mole fraction)

3. Apply Dalton's Law

Since we're not given the moles of CO2, we can't calculate its partial pressure directly. However, we know the total pressure (1.05 ATM) and the mole fractions of the other gases.

4. Assume Ideal Gas Behavior

We'll assume the gases behave ideally. This means the partial pressure of each gas is proportional to its mole fraction.

5. Solve for the Partial Pressure of CO2

* Let P(CO2) be the partial pressure of carbon dioxide.

* Total pressure (Ptotal) = P(N2) + P(H2) + P(CO2)

* P(CO2) = Ptotal - P(N2) - P(H2)

* P(CO2) = Ptotal - (mole fraction of N2 * Ptotal) - (mole fraction of H2 * Ptotal)

* P(CO2) = 1.05 ATM - (0.75 * 1.05 ATM) - (0.25 * 1.05 ATM)

* P(CO2) = 0 ATM

Conclusion

The partial pressure of carbon dioxide in this container is 0 ATM. This means there is likely no carbon dioxide present in the container.