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Calculate the mass of propylene glycol (C3H8O₂) that must be added to 0.340 kg of water to reduce the vapor pressure by 2.88 torr at 40°C. (Vapor pressure of water at 40°C = 55.37 torr)

Calculate the mass of propylene glycol (C3H8O₂) that must be added to 0.340 kg of water to reduce the vapor pressure by 2.88 torr at 40°C. (Vapor pressure of water at 40°C = 55.37 torr)

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Tutorial Chapter 3.pdf user/Downloads/Tutorial%20Chapter%203.pdf Read aloud Tutorial Chapter 1. Calculate the mass of propylene glycol (C3H8O₂) that must be added to 0.340 kg of water to reduce the vapor pressure by 2.88 torr at 40°C. (Vapor pressure of water at 40°C = 55.37 torr) 2. Ethanol (C₂H5OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 J/gK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C. II + 3. The phase diagram of sulfur is shown below. Determine the number of triple points, the most stable allotrope of sulfur at normal conditions and describe the outcome when sulfur at 1 atm is heated from 80°C to 200°C. P (atm) 1 of 1 i 1.0 154°C 1288 atm Rhombic Liquid - Monoclinic A 10-4 atm 10-5; atm Vapor 95.4°C 119°C 1 (°C) 28°C Partly cloudy C
Transcribed Image Text:Tutorial Chapter 3.pdf user/Downloads/Tutorial%20Chapter%203.pdf Read aloud Tutorial Chapter 1. Calculate the mass of propylene glycol (C3H8O₂) that must be added to 0.340 kg of water to reduce the vapor pressure by 2.88 torr at 40°C. (Vapor pressure of water at 40°C = 55.37 torr) 2. Ethanol (C₂H5OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 J/gK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C. II + 3. The phase diagram of sulfur is shown below. Determine the number of triple points, the most stable allotrope of sulfur at normal conditions and describe the outcome when sulfur at 1 atm is heated from 80°C to 200°C. P (atm) 1 of 1 i 1.0 154°C 1288 atm Rhombic Liquid - Monoclinic A 10-4 atm 10-5; atm Vapor 95.4°C 119°C 1 (°C) 28°C Partly cloudy C
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