1. Suppose o2, n2 and Ar were placed at 1.00 atm and 273 K in closed containers. A tiny hole is opened in each container, allowing each gas to diffuse into another container filled with neon gas. What is the ratio of the rate of diffusion of nitrogen to the rate of diffusion of oxygen? Is this greater than, less than, or the same as the ratio of the rates of effusion for the two gases?

To determine the ratio of the rate of diffusion of nitrogen (N2) to the rate of diffusion of oxygen (O2), we can use Graham's Law of Diffusion. According to Graham's Law, the rate of diffusion or effusion of a gas is inversely proportional to the square root of its molar mass.

First, we need to calculate the molar masses of nitrogen and oxygen:

- Molar mass of nitrogen (N2) = 28.0134 g/mol
- Molar mass of oxygen (O2) = 31.9988 g/mol

Next, we can calculate the square roots of their molar masses:

- Square root of the molar mass of nitrogen (N2) = √28.0134 ≈ 5.292 g/mol^(1/2)
- Square root of the molar mass of oxygen (O2) = √31.9988 ≈ 5.656 g/mol^(1/2)

Now, we can find the ratio of the rate of diffusion of nitrogen to the rate of diffusion of oxygen. Since diffusion rates are inversely proportional to the square root of molar mass, the ratio can be calculated as:

Ratio of diffusion rates = (Square root of molar mass of oxygen) / (Square root of molar mass of nitrogen)

= 5.656 g/mol^(1/2) / 5.292 g/mol^(1/2)

≈ 1.069

The ratio of the rate of diffusion of nitrogen to the rate of diffusion of oxygen is approximately 1.069.

To determine if this ratio is greater than, less than, or the same as the ratio of the rates of effusion for the two gases, we need to check if there are any differences between diffusion and effusion. Diffusion occurs when gas molecules move from areas of high concentration to low concentration, while effusion refers to the escape of gas molecules through a small opening into a vacuum.

In this particular scenario, the gases are diffusing into a container filled with neon gas, which implies that the gases are allowed to mix. Since there is no mention of a vacuum or a small opening, we can assume that the gases diffuse into the container rather than effusing.

Therefore, the ratio of the rates of diffusion and the ratio of the rates of effusion will be the same, i.e., 1.069.