Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25^∘ C . The

step 1 All right, guys, problem 58 of chapter 11. So, casually solubility of O2 in water at a partial p

Calculate the solubility of O2 in water at a partial...

Calculate the solubility of $\mathrm{O}_{2}$ in water at a partial pressure of $\mathrm{O}_{2}$ of 120 torr at $25^{\circ} \mathrm{C}$ . The Henry's law constant for $\mathrm{O}_{2}$ is $1.3 \times 10^{-3} \mathrm{mol} / \mathrm{L} \cdot$ atm for Henry's law in the form $C=k P$ where $C$ is the gas concentration $(\mathrm{mol} / \mathrm{L})$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Unit Conversion

Ensuring that units match is critical in applying Henry's Law correctly. When the Henry's law constant is provided in one set of units (such as atm), any pressure value given in a different unit (such as torr) must be converted appropriately. For instance, converting torr to atm is necessary since 1 atm is equal to 760 torr.

Gas Solubility

Gas solubility in a liquid depends on the gas’s partial pressure and the specific interactions between the gas and the liquid, as quantified by the Henry's law constant. Understanding gas solubility is important in fields like environmental science, chemical engineering, and physiology, where the behavior of gases in liquids can have significant practical implications.

Henry's Law

Henry's Law states that the concentration of a dissolved gas in a liquid is directly proportional to its partial pressure in equilibrium with the liquid. This law is expressed as C = kP, where C is the concentration of the gas, k is the Henry's law constant, and P is the partial pressure of the gas. This principle is fundamental in understanding and calculating gas solubility in various solvents.

Transcript

Please give Ace some feedback