The Henry's law constant for O2 is 1.3 ×10^-3 M / atm at...

The Henry's law constant for $\mathrm{O}_{2}$ is $1.3 \times 10^{-3} \mathrm{M} /$ atm at $25^{\circ} \mathrm{C}$. Assuming ideal solution behavior, what mass of oxygen would be dissolved in a 40-L aquarium at $25^{\circ} \mathrm{C}$, assuming an atmospheric pressure of $1.00 \mathrm{atm}$, and that the partial pressure of $\mathrm{O}_{2}$ is 0.21 atm?

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Key Concepts

Molar Mass

Molar mass is the mass per mole of a substance and is used to convert between the number of moles and the mass of a substance. After using Henry's Law to calculate the moles of gas dissolved, the molar mass allows one to determine the corresponding mass, which is often the desired quantity in practical calculations.

Molarity

Molarity is a measure of concentration defined as the number of moles of a solute per liter of solution. In the context of gas solubility, it helps in quantifying the amount of gas dissolved in a liquid once Henry's Law has been applied.

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 the gas phase. This relationship is typically expressed as C = k_H * P, where C is the concentration of the gas, k_H is the Henry's law constant, and P is the partial pressure of the gas. It is a key concept for understanding gas solubility in liquids under given conditions.

Partial Pressure

Partial pressure refers to the pressure that a particular gas in a mixture would exert if it occupied the entire volume alone. It is an important parameter in determining how much of a gas will dissolve in a liquid when applying Henry's Law, as only the gas's own pressure influences its solubility.

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