Answer:
The balanced chemical equation:
![C_6H_5OH(s)+7O_2(g)\rightarrow 6CO_2(g)+3H_2O(g)](https://tex.z-dn.net/?f=C_6H_5OH%28s%29%2B7O_2%28g%29%5Crightarrow%206CO_2%28g%29%2B3H_2O%28g%29)
Heat of combustion per gram of phenol is 32.454 kJ/g
Heat of combustion per gram of phenol is 3,050 kJ/mol
Explanation:
![C_6H_5OH(s)+7O_2(g)\rightarrow 6CO_2(g)+3H_2O(g)](https://tex.z-dn.net/?f=C_6H_5OH%28s%29%2B7O_2%28g%29%5Crightarrow%206CO_2%28g%29%2B3H_2O%28g%29)
Heat capacity of calorimeter = C = 11.66 kJ/°C
Initial temperature of the calorimeter = ![T_1= 21.36^oC](https://tex.z-dn.net/?f=T_1%3D%2021.36%5EoC)
Final temperature of the calorimeter = ![T_2= 26.37^oC](https://tex.z-dn.net/?f=T_2%3D%2026.37%5EoC)
Heat absorbed by calorimeter = Q
![Q=C\times \Delta T](https://tex.z-dn.net/?f=Q%3DC%5Ctimes%20%5CDelta%20T)
Heat released during reaction = Q'
Q' = -Q ( law of conservation of energy)
Energy released on combustion of 1.800 grams of phenol = Q' = -(58.4166 kJ)
Heat of combustion per gram of phenol:
![\frac{Q'}{1.800 g}=\frac{-58.4166 kJ}{1.800 g}=32.454 kJ/g](https://tex.z-dn.net/?f=%5Cfrac%7BQ%27%7D%7B1.800%20g%7D%3D%5Cfrac%7B-58.4166%20kJ%7D%7B1.800%20g%7D%3D32.454%20kJ%2Fg)
Molar mass of phenol = 94 g/mol
Heat of combustion per gram of phenol:
![\frac{Q'}{\frac{1.800 g}{94 g/mol}}=\frac{-58.4166 kJ\times 94 g/mol}{1.800 g}=3,050 kJ/mol](https://tex.z-dn.net/?f=%5Cfrac%7BQ%27%7D%7B%5Cfrac%7B1.800%20g%7D%7B94%20g%2Fmol%7D%7D%3D%5Cfrac%7B-58.4166%20kJ%5Ctimes%2094%20g%2Fmol%7D%7B1.800%20g%7D%3D3%2C050%20kJ%2Fmol)