A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/?C. The temperature of the calorimeter plus contents increased from 21.36?Cto 26.37?C. Part A
Write a balanced chemical equation for the bomb calorimeter reaction.
Part B:
What is the heat of combustion per gram of phenol?Part C:
Per mole of phenol?

The balanced chemical equation:

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:

Heat capacity of calorimeter = C = 11.66 kJ/°C

Initial temperature of the calorimeter =

Final temperature of the calorimeter =

Heat absorbed by calorimeter = Q

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:

Molar mass of phenol = 94 g/mol

Heat of combustion per gram of phenol:

the maximum mass of nh3 is nh3 in grams