19.4a & c An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermalequilibrium at 10.0°C. Two metallic blocks are placed into the water. One is a 100.0-g piece of copper at 50.0°C. The otherhas a mass of 70.0 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of20.0°C.FigureSubstanceElemental solidsAluminumBerylliumCadmiumCopperGermaniumGoldIronLeadSpecific Heats of Some Substances at 25°C and Atmospheric PressureSpecific Heat(J/kg. °C)Elemental SolidsSiliconSilver9001 830230387322129448128703234Other Solids(a) Determine the specific heat of the unknown sample.J/(kg• °C)SubstanceOther solidsBrassGlassIce (-5°C)MarbleWoodLiquidsAlcohol (ethyl)MercuryWater (15°C)GasSteam (100°C)Liquids and GasSpecific Heat(J/kg. °C)3808372 0908601 7002 4001404 1862010Specific heats of some substances at 25°C and atmospheric pressure are provided. Refer to the adjacent tables forspecific values.i (b) Using the data in the table above, can you make a positive identification of the unknown material?YesNoCan you identify a possible material?YesNo(c) Explain your answers for part (b).

Answered: Image /qna-images/answer/f926f4c6-72e6-4c1c-b069-8696bb495e42.jpg

An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10.0°C. Two metallic blocks are placed into the water. One is a 100.0-g piece of copper at 50.0°C. The other has a mass of 70.0 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20.0°C.

An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10.0°C. Two metallic blocks are placed into the water. One is a 100.0-g piece of copper at 50.0°C. The other has a mass of 70.0 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20.0°C.

Physics for Scientists and Engineers: Foundations and Connections

1st Edition

ISBN:9781133939146

Author:Katz, Debora M.

Publisher:Katz, Debora M.

Chapter21: Heat And The First Law Of Thermodynamics

Section: Chapter Questions

Problem 21PQ

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Question

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19.4

a & c

An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal
equilibrium at 10.0°C. Two metallic blocks are placed into the water. One is a 100.0-g piece of copper at 50.0°C. The other
has a mass of 70.0 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of
20.0°C.
Figure
Substance
Elemental solids
Aluminum
Beryllium
Cadmium
Copper
Germanium
Gold
Iron
Lead
Specific Heats of Some Substances at 25°C and Atmospheric Pressure
Specific Heat
(J/kg. °C)
Elemental Solids
Silicon
Silver
900
1 830
230
387
322
129
448
128
703
234
Other Solids
(a) Determine the specific heat of the unknown sample.
J/(kg• °C)
Substance
Other solids
Brass
Glass
Ice (-5°C)
Marble
Wood
Liquids
Alcohol (ethyl)
Mercury
Water (15°C)
Gas
Steam (100°C)
Liquids and Gas
Specific Heat
(J/kg. °C)
380
837
2 090
860
1 700
2 400
140
4 186
2010
Specific heats of some substances at 25°C and atmospheric pressure are provided. Refer to the adjacent tables for
specific values.
i

(b) Using the data in the table above, can you make a positive identification of the unknown material?
Yes
No
Can you identify a possible material?
Yes
No
(c) Explain your answers for part (b).

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