Question 3 A chemist accidentally leaves a 300.0 g sample of benzene on an activated hotplate. The benzene heats up from 25 °C to 100 °C and when the chemist returns, is surprised to see the benzene is gone. How much heat (in kJ to two decimal places) is required for this process?

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Heating curve data with the question.
Heating curve data for some substances
Name
Acetone
Ammonia
Benzene
Methanol
Propane
m.m.
58.08
17.03
78.11
32.04
44.1
Tf
-94.9
5.538
Tb
-77.65 -33.33
-97.5
56.08
80.08
64.5
-187.62 -42.11
AHfus
5.77
5.66
9.87
3.215
3.5
AHvap
29.1
23.33
30.72
35.21
19.04
*Temperatures in °C; enthalpies in kJ mol; specific heats in J g-¹ °C-1
Cs
1.653
1.10
CI
2.409 1.283
2.061
1.741
Cg
2.531
1.703
1.16
1.376
2.025 1.669
Transcribed Image Text:Heating curve data for some substances Name Acetone Ammonia Benzene Methanol Propane m.m. 58.08 17.03 78.11 32.04 44.1 Tf -94.9 5.538 Tb -77.65 -33.33 -97.5 56.08 80.08 64.5 -187.62 -42.11 AHfus 5.77 5.66 9.87 3.215 3.5 AHvap 29.1 23.33 30.72 35.21 19.04 *Temperatures in °C; enthalpies in kJ mol; specific heats in J g-¹ °C-1 Cs 1.653 1.10 CI 2.409 1.283 2.061 1.741 Cg 2.531 1.703 1.16 1.376 2.025 1.669
Question 3
A chemist accidentally leaves a 300.0 g sample of benzene on an activated hotplate. The benzene
heats up from 25 °C to 100 °C and when the chemist returns, is surprised to see the benzene is gone.
How much heat (in kJ to two decimal places) is required for this process?
Transcribed Image Text:Question 3 A chemist accidentally leaves a 300.0 g sample of benzene on an activated hotplate. The benzene heats up from 25 °C to 100 °C and when the chemist returns, is surprised to see the benzene is gone. How much heat (in kJ to two decimal places) is required for this process?
Expert Solution
Step 1

Given 

Mass of Sample (m) = 300 g 3001000=0.3 kg

Initial temperature (t1) = 250C= (25+273)K=298 K

Final Temperature (t2) =1000C= (100+273)K=373K

Difference (t) =

(t2-t1)=(373-298)K            = 75KSpecific heat capacity for liquid benzene =1.70 KJ/Kg K

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