A 1.800- g sample of solid phenol ( C 6 H 5 O H ( s ) ) was burned in a bomb cal

Question

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? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol 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. 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. 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. 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? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol Part A Write a balanced chemical equation for the bomb calorimeter reaction.
Part B: What is the heat of combustion per gram of phenol? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol Part A Write a balanced chemical equation for the bomb calorimeter reaction.
Part B: What is the heat of combustion per gram of phenol? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol Part A Write a balanced chemical equation for the bomb calorimeter reaction.
Part B: What is the heat of combustion per gram of phenol? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol Part A Write a balanced chemical equation for the bomb calorimeter reaction.
Part B: What is the heat of combustion per gram of phenol? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol Part A Write a balanced chemical equation for the bomb calorimeter reaction.
Part B: What is the heat of combustion per gram of phenol? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol 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? ?? kJ/g
Part C: Per mole of phenol? ?? kJ/mol

Explanation / Answer

Part A:

C6H5OH + 7 O2 = 6 CO2 + 3 H2O
Part B:

Heat liberated per gram Q= H*Delta T / w

H= heat capacity of calorimeter.

Delta T = T2-T1 .        T2>T1

w= mass of phenol

= 11.66*(26.37-21.36)/1.8

= - 32.28 Kj/g

Part c:

Heat liberated per mole Q= H*Delta T / n

n= no of moles = 1.8/94.11 = 0.019126554 mole.

= 11.66*(26.37-21.36)/ 0.019126554

= - 3054.21458 KJ/mol.

note:    "-" indicates liberation of heat in the reaction.

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