Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water in atmospheres at 0 °C is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 * 10-3 mol>L.

검증된 단계별 안내

First, convert the required oxygen concentration from mg/L to mol/L. To do this, divide the given concentration by the molar mass of oxygen (32 g/mol).

Next, compare the required concentration to the solubility of oxygen at 0 °C and 1 atm. The solubility tells us how many moles of oxygen can be dissolved in 1 L of water under these conditions.

Since the required concentration is higher than the solubility, we need to increase the partial pressure of oxygen above the water. According to Henry's law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

Calculate the ratio of the required concentration to the solubility. This ratio is equal to the ratio of the required partial pressure to 1 atm.

Finally, multiply the ratio by 1 atm to find the required partial pressure of oxygen above the water.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This principle is crucial for understanding how the concentration of oxygen in water relates to its partial pressure in the atmosphere.

Gas Solubility

Gas solubility refers to the maximum amount of gas that can dissolve in a solvent at a specific temperature and pressure. In this case, the solubility of O2 in water at 0 °C and 1 atm is given as 2.21 * 10^-3 mol/L, which helps determine how much oxygen can be dissolved to meet the survival needs of fish.

Molar Concentration

Molar concentration, or molarity, is a measure of the concentration of a solute in a solution, expressed in moles per liter (mol/L). To find the required partial pressure of oxygen to achieve a concentration of 4 mg/L, it is essential to convert this mass concentration into molarity using the molar mass of oxygen.