Question

The circles illustrate a mixture of diatomic nitrogen (N2) and oxygen (O2) molecules inside of flasks. Each flask has the same volume. The nitrogen molecules are shown in blue and the oxygen molecules are shown in red.

Answer 1

The relationship described by Dalton's Law helps explain how changes in the number of molecules (moles) of a specific gas in a mixture can influence its partial pressure. As you increase the number of moles of a gas, its partial pressure will increase proportionally, assuming ideal gas behavior and constant conditions.

Dalton's Law of Partial Pressures states that in a mixture of gases, the total pressure is the sum of the partial pressures of each individual gas. The partial pressure of a specific gas is directly proportional to the number of moles of that gas present in the mixture, assuming ideal gas behavior.

In the given scenario:

Flask B has the greater partial pressure of nitrogen:

This implies that there is a higher number of moles of nitrogen gas in Flask B compared to the other flask(s). According to Dalton's Law, increasing the number of moles of a gas in a mixture will result in a proportional increase in its partial pressure, assuming other conditions remain constant.

Flask D has the greatest partial pressure of oxygen:

Similarly, this suggests that Flask D contains a higher number of moles of oxygen gas compared to the other flask(s). Again, Dalton's Law indicates that increasing the number of moles of a gas will lead to a proportional increase in its partial pressure.

Answer 2

• Flask B has the greater partial pressure of nitrogen
• Flask D has the greatest partial pressure of oxygen

The relationship between partial pressure and the number of molecules of a specific gas in a mixture is described by Dalton's Law of Partial Pressures. The partial pressure of a gas in a mixture is directly proportional to the number of moles of that gas, assuming ideal gas behavior.

If you increase the number of molecules (moles) of a gas in a mixture, its partial pressure will increase proportionally, assuming other conditions remain constant.