A 1.800-g sample of solid phenol (C6H5OH(s)) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/?

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?

Answers

The balanced chemical equation:

C_6H_5OH(s)+7O_2(g)rightarrow 6CO_2(g)+3H_2O(g)

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)

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

Initial temperature of the calorimeter = T_1= 21.36^oC

Final temperature of the calorimeter = T_2= 26.37^oC

Heat absorbed by calorimeter = Q

Q=Ctimes Delta T

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

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 kJtimes 94 g/mol}{1.800 g}=3,050 kJ/mol

well i think it's b

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