Ch.14 - Solutions

Tro - Chemistry: A Molecular Approach 6th Edition

Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217당신이 사용하는 게 아니라요?교과서 변경

Tro 6th Edition

Ch.14 - Solutions

문제 111

14장, 문제 111

A saturated solution forms when 0.0537 L of argon, at a pressure of 1.0 atm and temperature of 25 °C, is dissolved in 1.0 L of water. Calculate the Henry's law constant for argon.

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Identify the given values: volume of argon gas (V_gas) = 0.0537 L, pressure (P) = 1.0 atm, temperature (T) = 25 °C, and volume of water (V_water) = 1.0 L.

Convert the temperature from Celsius to Kelvin using the formula: T(K) = T(°C) + 273.15.

Use the ideal gas law, PV = nRT, to calculate the number of moles of argon gas (n). Here, R is the ideal gas constant (0.0821 L·atm/mol·K).

Determine the concentration of argon in the solution by dividing the number of moles of argon by the volume of water in liters.

Apply Henry's Law, which states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid: C = kH * P, where C is the concentration of the gas, kH is Henry's law constant, and P is the pressure. Rearrange to solve for kH: kH = C / P.

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주요 개념

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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 relationship can be expressed mathematically as C = kH * P, where C is the concentration of the gas in the liquid, kH is the Henry's law constant, and P is the partial pressure of the gas.

Saturation Concentration

A saturated solution is one in which the maximum amount of solute has been dissolved in the solvent at a specific temperature and pressure. In the context of gases, this means that the concentration of the gas in the liquid phase is at its limit, and any additional gas will not dissolve but will remain in the gaseous phase.

Units of Henry's Law Constant

The Henry's law constant (kH) can be expressed in various units depending on the context, such as mol/(L·atm) or atm/(mol/L). Understanding the units is crucial for correctly calculating and interpreting the constant, as it relates the concentration of the dissolved gas to its partial pressure in the gas phase.

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