Question

In: Chemistry

In an adiabatic, constant-volume bomb calorimeter, a combustion of 0.7362g of naphthalene (C10H8) caused the temperature...

In an adiabatic, constant-volume bomb calorimeter, a combustion of 0.7362g of naphthalene (C10H8) caused the temperature to rise of 5.707 Celcius. The final temperature was 298.000K. The heat capacity of the calorimeter, Ccal was 10290 J/K . (Note: this value of Ccal includes the contribution from water.) The molar enthalpies of formation of CO2(g) and H2O(l) are: -393.522 kJ/mol, -285.830 kJ/mol, respectively Mm(C)= 12.01 g/mol and Mm(H)= 1.001 g/mol.

a.) Calculate deltaUc , deltaUcm , delta Hcm for this combustion reaction.

b.) What are delta Hf and delta Hfm of naphthalene?

Solutions

Expert Solution

Note: FYI, the values calculated here do not agree with the actual scientific data. There must be some error in either temperature rise(5.707) or the heat capacity of the calorimeter.


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