At 1 atm and 0°C, the densitiesof water and ice are 1.00g / cm-3and 0.924g / cm-3 , respectively .If the latent heat of fusion of thenormal melting point of water is316.9 J/g, what is the freezingpressure of water at -10 ° C ? (R- 82.06 cm.atm.mol - 1.K -1,R =1.987 cal . mol - 1.K - 1)

Given data: T1= 00C P1 = 1 atm Density of water = 1 g/cm3 Density of ice = 0.924 g/cm3 Latent heat…

Answered: At 1 atm and 0 ° C , the densities of…

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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(w/ complete process pls) Determine the enthalpy change when 1 mol of SO2 gas is cooled from 538oC to -101oC at atmospheric pressure. The data are:Boiling Point: -5oCMelting Point: -75.5oCLatent Heat of Vaporization: 24,940 J/molLatent heat of Fusion: 7,401 J/molAverage Cp of liquid SO2: 1.28 J/moloCAverage Cp of solid SO2: 0.958 J/moloCCp of gaseous SO2: (kindly provide Cp of gaseous SO2; could be from internet or books)
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If ice homogeneously nucleates at -57.8°C, calculate the critical radius given values of -3.1 x 108 J/m³ and 25 x 10-3 J/m2, respectively, for the latent heat of fusion and the surface free energy 0.9854 x 10-10 m O 0.1284 x 10-5 m O 0.5981 x 10-11 m O 0.7618 x 10-9 m
The molar enthalpy of fusion of ice at 0°C is 6.02 kJ mol-'; the molar heat capacity of undercooled water is 75.3 J mol-1 K-!, (a) One mole of undercooled water at -10°C is induced to crystallize in a heat-insulated vessel. The result is a mixture of ice and water at 0°C. What frac- tion of this mixture is ice? (b) Calculate AS for the system.
Part II: Calculate the following two quantities for 5.00 mol of an ideal gas with Cv.m = 5/2 R that is heated at constant volume from 300. K to 400. K by a single irreversible transfer of heat to the initial state. 9irrev T ( dqrev AS = and T
At the triple point of water, 0.01C; ice, liquid water and water vapor are in equilibrium under a pressure of 4.58 mm Hg. At this temperature, the heat of fusion of ice is 1436 cal/mol and the heat of vaporization is 10,767 cal/mol. From these data, find the entropy change for the sublimation of ice. Select the correct response: 5.26 cal/K 34.14 cal/K 39.4 cal/k 44.7 cal/K
The change of heat capacity with temperature for solid aluminum is as follows:Cp(J/K mol) = 20.67 + 12.38 x10-3 T (in the range of 25 -700 °C )If 1 mol of Aluminum is heated from 25°C to 700°C, what will be the entropy change?
Coaxial and parallel to each other, full and semicircle as seen in the figure determine the heat transfer that occurs by radiation between the two surfaces in its form. Assume that the surfaces only exchange radiation with each other. T1 = 700 °C; ε1=0.8; T2 = 20 °C; ε2=0.4.
For substance A, it is known that the vapor pressure at 300K is 100kPa. It is also known that the boiling point temperature is 340K at 150 kPa. Other given information about substance A: Cpl= 200 J/mol.K and Cpv = 180 J/mol.K c) Using the correlation developed in part a), determine the latent heat of vaporization of substance A in kJ/kmol d) 2 mol of substance A goes through a process where its temperature changes from 400K to 300K at constant pressure 150kPa. i) What phase is present initially? ii) What phase is present at the final state? iii) Determine the total amount of energy transferred (in kJ) through the process and state whether the energy is transferred to or from the substance.

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