A chemist carefully measures the amount of heat needed to raise the temperature of a 2.00kg sample of C2H2Cl2 from 6.3°C to 16.5°C. The experiment shows that ×2.25104J of heat are needed. What can the chemist report for the molar heat capacity of C2H2Cl2? Be sure your answer has the correct number of significant digits.

Question
Asked Nov 6, 2019

A chemist carefully measures the amount of heat needed to raise the temperature of a 2.00kg sample of C2H2Cl2 from 6.3°C to 16.5°C. The experiment shows that ×2.25104J of heat are needed. What can the chemist report for the molar heat capacity of C2H2Cl2? Be sure your answer has the correct number of significant digits.

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Step 1

Given data

Mass of C2H2Cl2 = 2.0kg

Total heat = 2.25x104 J

Temperature difference = (16.5 - 6.3)°C

Step 2

The equation for heat needed

Q=mcAT
where
m is the number of moles
c is the molar heat capacity
AT is the temperature change
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Q=mcAT where m is the number of moles c is the molar heat capacity AT is the temperature change

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Step 3

No of moles of the substance provid...

given mass
no of moles=
molar mass
2000
97
-20.619
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given mass no of moles= molar mass 2000 97 -20.619

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