From the given, calculate: 1. Melt water temperature change 2. Heat lost by water (show all calculations)
From the given, calculate: 1. Melt water temperature change 2. Heat lost by water (show all calculations)
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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Question
From the given, calculate:
1. Melt water temperature change
2. Heat lost by water
(show all calculations)
Transcribed Image Text:Data Sheet
Time (s)
T (°C)
Time (s)
T (°C)
Time (s)
T (°C)
40°C
180
16.4°C
360
4.8°C
20
39.9°C
39.6°C
200
12.2°C
380
4.5°C
4.2°C
40
220
10.4°C
400
60
80
37°C
33.6°C
420
440
240
7.9°C
7.6°C
4°C
4°C
260
100
30.3°C
280
5.8°C
460
4°C
4°C
5.5°C
5°C
4.9°C
120
26.1°C
300
480
140
160
22.4°C
320
500
520
4°C
18°C
340
4°C
Hot water volume,V1
Hot water initial temperature, T1
Final water volume,V2
Final water temperature, T2
100mL
155.6 mL
40°C
4°C
Given: 25g ice cubes
100g water at 40 °C (p40 = 0.9932 g/mL).
Transcribed Image Text:Hot water mass: m hot = V1'p
%3D
4
Total water mass: m total = V2°p
Melt water mass: m melt = m total – m hot
Hot water temperature change: AT hot = T2– T1
Melt water temperature change: AT melt = T2 – 0.0 °C
Heat lost by hot water: q hot = Cp · m hot · AT hot
Heat gained by melt water: q melt = Cp · m melt · AT melt
Heat absorbed by melting ice: q fusion = (g hot + q melt)
9.
fusion
Heat absorbed per mole: ² H fus
molesmelt
% difference from accepted value:
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