Why were we not able to simply use the specific heat capacity of water, 4.184 J/g°C? Procedure:1. Set up the calorimeter apparatus, as shown.2. Obtain the mass of the paraffin wax before it is lit and record it in the data table below.3. Measure 100.0 mL of water and add it to the calorimeter. Record the mass of the calorimeterand water together. Record the temperature of the water, as accurately as possible.4. Light the candle and immediately place it under the can. Adjust the height of the can so that thetip of the flame is 1cm or less below the can.5. Occasionally, stir the water gently. Watch for the temperature to increase by roughly 10°Cabove the starting temperature. Record the maximum temperature reached as accurately aspossible.6. Blow out the candle and remove it from the base of the calorimeter. Allow it to cool.

Given that: Volume of water used = 100 mL specific heat capacity of water = 4.184 J/g oC Change in…

Answered: Why were we not able to simply use the…

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Why were we not able to simply use the specific heat capacity of water, 4.184 J/g°C?

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Energy

Section: Chapter Questions

Problem 28A

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Question

Why were we not able to simply use the specific heat capacity of water, 4.184 J/g°C?

Procedure:
1. Set up the calorimeter apparatus, as shown.
2. Obtain the mass of the paraffin wax before it is lit and record it in the data table below.
3. Measure 100.0 mL of water and add it to the calorimeter. Record the mass of the calorimeter
and water together. Record the temperature of the water, as accurately as possible.
4. Light the candle and immediately place it under the can. Adjust the height of the can so that the
tip of the flame is 1cm or less below the can.
5. Occasionally, stir the water gently. Watch for the temperature to increase by roughly 10°C
above the starting temperature. Record the maximum temperature reached as accurately as
possible.
6. Blow out the candle and remove it from the base of the calorimeter. Allow it to cool.

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9.41 Under what conditions does the enthalpy change equal the heat of a process?
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Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?
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