Observation - Alcohol No. Of Carbon atoms per Alcohol Initial Mass Final Mass?

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Observation

Alcohol        No. Of Carbon atoms per Alcohol        Initial Mass        Final Mass?
Mass (g)        Initial Temperature        Final Temperature?
Temperature        ?H/g (kJ/g)        ?H/mol (kJ/mol)
Methanol
1)
2)
3)
Average)        1        
243.34g
238.59g
236.46g        
238.59g
236.46g
233.94g        
4.75g
2.13g
2.52g        
17ºC
16ºC
18ºC        
52ºC
54ºC
50ºC        
34ºC
35ºC
38ºC        
3.006
6.901
6.333        
96.2
220.8
202.7
211.8
Ethanol
1)
2)
3)
Average)        2        
234.96g
217.36g
205.17g        
232.2g
213.79g
201.02g        
2.76g
3.57g
4.15g        
16ºC
17ºC
19ºC        
51ºC
60ºC
52ºC        
35ºC
43ºC
33ºC        
5.326
5.059
3.340        
245.0
232.7
153.6
238.9
Propanol
1)
2)
3)
Average)        3        
203.61g
201.35g
242.21g        
201.35g
199.54g
240.52g        
2.26g
1.81g
1.69g        
19ºC
18ºC
23ºC        
50ºC
50ºC
54ºC        
31ºC
32ºC
31ºC        
5.761
7.425
7.704
        
345.7
445.5
462.2
453.85
Butanol
1)
2)
3)
Average)        4        
197.7g
196.26g
194.63g        
196.26g
194.63g
192.31g        
1.44g
1.63g
2.32g        
15ºC
19ºC
18ºC        
47ºC
51ºC
50ºC        
32ºC
32ºC
32ºC        
9.333
8.245
5.793        
690.6
610.1
428.7
650.35

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So as you can see by my results Butanol has the highest enthalpy of combustion.?

 To calculate the energy produced or lost during these experiments I used the formula:

    DH= mass of water x 4.2 x Dt  = J/g

                   DM

  This is the formula m x  x t where m is the mass of the water and c is the energy needed to heat up 1kg of the substance 1°C.

  We then divide this by 1000 to get the answer in kJ/mol ...

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