Hot water mass: m hot = V 1"p Total water mass: m total = V zp * 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 = (q hot + q meli) fsion Heat absorbed per mole: * H fas molesmelt % difference from accepted value:
Hot water mass: m hot = V 1"p Total water mass: m total = V zp * 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 = (q hot + q meli) fsion Heat absorbed per mole: * H fas molesmelt % difference from accepted value:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
From the given, calculate:
1. Heat gained by melt water
2. ∆Hfus
(show all calculations)
Transcribed Image Text:Time (s)
T (°C)
Time (s)
T (°C)
Time (s)
T (°C)
40°C
180
20.1°C
360
4.6°C
20
39.6°C
200
17.5°C
380
4.6°C
40
39.2°C
220
13.9°C
400
4°C
60
37°C
240
10°C
420
4°C
80
33.7°C
260
9.8°C
440
4°C
100
31.4°C
280
9.1°C
460
4°C
120
29.6°C
300
8.3°C
480
4°C
140
25.3°C
320
5°C
500
4°C
160
22°C
340
4.8°C
520
4°C
Hot water volume, V,
Final water volume, V2
125 mL
100 mL
Hot water initial
40 °C
Final water
18 °C
temperature, T,
temperature, T2
p40(H20) = 0.9932 g/mL
T.V. = 6.01 kJ/mol
Cp of water = 4.184 J/g°C
% difference from accepted value (% error) = T.V. - E.V. x 100
Moles melt = m melt /MMH,0
T.V.
Heat absorbed per mole = q fusion/ moles melt (E.V.) =
kI/mole (1k) =100OJ)
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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