Скачать с ютуб ⚗️ Calculating the Vapor Pressure of a Solution using Raoult’s law (Question 1) в хорошем качестве

⚗️ Calculating the Vapor Pressure of a Solution using Raoult’s law (Question 1)

✔ https://StudyForce.com ✔ https://Biology-Forums.com ✔ Ask questions here: https://Biology-Forums.com/index.php?... Follow us: ▶ Facebook:   / studyforceps   ▶ Instagram:   / studyforceonline   ▶ Twitter:   / studyforceps   Q1. Calculate the vapor pressure at 25 °C of a solution containing 99.5 g sucrose (C12H22O11) and 300.0 mL water. The vapor pressure of pure water at 25 °C is 23.8 torr. • Assume the density of water is (1.00 g∕mL) • Molar mass of sucrose is (342.3 g∕mol) Q2. Calculate the vapor pressure at 25 °C of a solution containing 55.3 g ethylene glycol (HOCH2CH2OH) and 285.2 g water. The vapor pressure of pure water at 25 °C is 23.8 torr. • Molar mass of sucrose is (62.07 g∕mL) Q3. A solution containing ethylene glycol and water has a vapor pressure of 7.88 torr at 10 °C. Pure water has a vapor pressure of 9.21 torr at 10 °C. What is the mole fraction of ethylene glycol in the solution? You are given the mass of sucrose and volume of water in a solution. You are also given the vapor pressure of pure water and asked to find the vapor pressure of the solution. The density of the pure water is also provided. Raoult’s law relates the vapor pressure of a solution to the mole fraction of the solvent and the vapor pressure of the pure solvent. Begin by calculating the amount in moles of sucrose and water. Calculate the mole fraction of the solvent from the calculated amounts of solute and solvent. Use Raoult’s law to calculate the vapor pressure of the solution. Calculate the number of moles of each solution component. Use the number of moles of each component to calculate the mole fraction of the solvent (H2O). Use the mole fraction of water and the vapor pressure of pure water to calculate the vapor pressure of the solution. The units of the answer are correct. The magnitude of the answer is about right because the calculated vapor pressure of the solution is just below that of the pure liquid, as expected for a solution with a large mole fraction of solvent.