CALCULATIONSDo the following with your experimental data.1 Calculate the amount of heat absorbed by the water. QH20 = m of H₂O x 4.184x (IT of H₂O) In this experiment you calculate specific heat of aluminum metal by calorimetry.Record your observations, complete Data table and perform calculations.Include both the numerical value and unit for each measurement and calculation.DatamassSpecific Heat of Aluminum metalSpecific Heat : C(J/g-°C)Initial temperature (°C):t₁Final temperature (°C) : t₂AT-t₂-t₁.Aluminum?20.5979.8°C)28.6°C51.1°cwater82.194.18426.2828.6°C2.4 cC

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Answered: Do the following with your experimental…

Do the following with your experimental data. 1 Calculate the amount of heat absorbed by the water. QH20 = m of H₂O x 4.184 x (IT of H₂O)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 14P

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Question

CALCULATIONS
Do the following with your experimental data.
1 Calculate the amount of heat absorbed by the water. QH20 = m of H₂O x 4.184
x (IT of H₂O)

In this experiment you calculate specific heat of aluminum metal by calorimetry.
Record your observations, complete Data table and perform calculations.
Include both the numerical value and unit for each measurement and calculation.
Data
mass
Specific Heat of Aluminum metal
Specific Heat : C(J/g-°C)
Initial temperature (°C):
t₁
Final temperature (°C) : t₂
AT-t₂-t₁.
Aluminum
?
20.59
79.8°C)
28.6°C
51.1°c
water
82.19
4.184
26.28
28.6°C
2.4 c
C

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