At 63.5 °C, the vapor pressure of H₂O is 175 torr, and that of ethanol (C₂H₅OH) is 400 torr. A solution is made by mixing equal masses of H₂O and C₂H₅OH. (b) Assuming ideal solution behavior, what is the vapor pressure of the solution at 63.5 °C?

검증된 단계별 안내

Calculate the moles of H_2O and C_2H_5OH using their respective molar masses.

Determine the mole fraction of each component in the solution.

Use Raoult's Law to calculate the partial vapor pressure of each component: P_i = X_i * P_i^0, where P_i is the partial pressure, X_i is the mole fraction, and P_i^0 is the pure component vapor pressure.

Add the partial pressures of H_2O and C_2H_5OH to find the total vapor pressure of the solution.

Ensure the solution behaves ideally by checking that the sum of the mole fractions equals 1.

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.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid phase at a given temperature. It reflects the tendency of particles to escape from the liquid phase into the vapor phase. The higher the vapor pressure, the more volatile the substance. In this question, the vapor pressures of pure water and ethanol at 63.5 °C are provided, which are essential for calculating the vapor pressure of the solution.

Raoult's Law

Raoult's Law states that the vapor pressure of a solvent in a solution is equal to the vapor pressure of the pure solvent multiplied by its mole fraction in the solution. This law applies to ideal solutions, where interactions between different molecules are similar to those between like molecules. In this scenario, Raoult's Law will be used to determine the vapor pressure of the mixed solution of water and ethanol.

Mole Fraction

Mole fraction is a way of expressing the concentration of a component in a mixture, defined as the number of moles of that component divided by the total number of moles of all components in the mixture. It is a crucial factor in Raoult's Law, as it helps to quantify the proportion of each component in the solution. In this case, calculating the mole fractions of water and ethanol will be necessary to find the overall vapor pressure of the solution.

At 63.5 °C, the vapor pressure of H2O is 175 torr, and that of ethanol (C2H5OH) is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH. (b) Assuming ideal solution behavior, what is the vapor pressure of the solution at 63.5 °C?