Final answer:
To determine the mass of CO2 gas with twice the partial pressure of N2 gas, we must first calculate the moles of N2 using its molar mass. Then, using the ratio of partial pressures and the molar mass of CO2, we can find the mass of the CO2 gas.
Step-by-step explanation:
The question involves finding the mass of CO₂ gas given that its partial pressure is twice that of N₂ gas, and we have 8.25g of N₂ gas in the container. To solve this problem, we can use the ideal gas law to find the moles of N₂, and then apply Dalton's Law of Partial Pressures which states that the total pressure of a gas mixture is the sum of the partial pressures of each component gas. Knowing the ratio of the partial pressures, we can calculate the moles and subsequently the mass of CO₂ gas.
We start by finding the moles of N₂ using its molar mass (28.02 g/mol). Next, we use the fact that the moles of CO₂ will be such that its partial pressure is twice that of N₂. Since the mass of a gas is directly proportional to the number of moles (given constant temperature and pressure conditions), and since we know the partial pressure relationship, we can use the molar mass of CO₂ (44.01 g/mol) to find the unknown mass of CO₂. However, without the temperature or volume of the container, we cannot determine the exact masses.