When 2.25 mg of anthracene, C₁4H₁0(s), was burned in a bomb calorimeter the temperature rose by 1.75K. Calculate the calorimeter constant. By how much will the temperature rise when 125 mg of phenol, C6H5OH(s) is burned in the calorimeter under the same conditions? AH combustion (anthracene) = -7061 kJ/mol
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
The mass of anthracene is .
The change in temperature is 1.75 K.
To find the calorimeter constant.
The heat of combustion is .
To calculate the temperature rise when the mass of phenol is 125 that is burned in the same bomb calorimeter.
Step by step
Solved in 4 steps with 11 images