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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Question
find the initial temperature of water, (e), (k), (l)
Transcribed Image Text:a hot metal is placed inside the calorimeter containing water. Inside the calorimeter, the hot
metal releases heat, which in turn is absorbed by the water and the calorimeter. The heat
released by the metal is equal to the heat absorbed by the calorimeter and the water based
on the equation shown:
Heat released (Q) = Heat absorbed (Q)
Heat released by metal = Heat absorbed by the calorinmeter + Heat absorbed by water
Qmetal
Qa + Qqrater
(mretal Cmatal ATmeta)
= (m.a Ca ATa) + (mate Cwatur ATrater)
= mass in grams
C = specific heat of a substance(theoretical)?
AT = change in temperature (Tf-Ti)
Where:
m
Table 4.1. Specific Heat of Common Metals.
Specific Heat – (C)
(Cal/g°C)
0.220
Metal
(J/g®C)
0.910
Aluminum
Brass
Copper
Iron (Fe)
Lead
Magnesium
Tin
0.380
0.390
0.090
0.092
0.460
0.108
0.130
0.031
1.050
0.382
0.243
0.054
1.000
Water
4.184
Transcribed Image Text:Results, and calculations: Complete the table below, using Fe as the metal
20g
105g
85g
Wt. of Calorimeter
Wt. of Calorimeter + water
Weight of Water
Initial temperature of water, (t)v
°C
(e) Initial temperature of aluminum calorimeter, (t)eal
(f) Initial temperature of metal (t)metal
(g) Weight of metal sample, mmetal
(h) Final temperature of water, (t)w
(i) Final temperature of calorimeter, (t)cal
G) Final temperature of metal
(k) Heat absorbed by the metal, gcal
(1) Heat absorbed by the water, gw
°C
100 °C
26 g
30.5 °C
30.5 °C
30.5 °C
Joule
Joule
(m) Experimental specific heat of metal sample
0.492 J/gC
(n) Theoretical specific heat of metal sample
0.460 J/gC
(0) Percent Error
7.0 %
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