Answer:
When a gaseous mixture of oxygen and nitrogen is maintained at a constant temperature, the following statements must be true regarding the two gases:
Each gas will have its own partial pressure: In a mixture of gases, each gas exerts a pressure known as its partial pressure. This means that oxygen and nitrogen will have their respective partial pressures in the mixture.
The total pressure of the mixture is the sum of the partial pressures: According to Dalton's law of partial pressures, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas in the mixture. Therefore, the total pressure of the oxygen-nitrogen mixture will be the sum of the partial pressures of oxygen and nitrogen.
The ratio of the partial pressures remains constant: At a constant temperature, the ratio of the partial pressures of oxygen and nitrogen will remain the same, provided the composition of the mixture remains unchanged. This is known as Dalton's law of partial pressures.
It's important to note that the specific properties and behaviors of oxygen and nitrogen can vary in different situations, but the above statements hold true for a gaseous mixture of oxygen and nitrogen at a constant temperature.