Consider the reaction C12H22011 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H20 (1) in which 11 g of sucrose, C12H22011, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C (including its water). The temperature inside the calorimeter was found to increase by 21.6 °C. Based on this information, what is the heat of this reaction per mole of sucrose? Enter your answer numerically, in terms of kJ/mol and to three significant figures.
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.
Given data:
Mass of sucrose m =11g,
Heat capacity C = 7.50 kJ/ o C
Change in temperature dT = 21.6 o C
Required data,
Molar mass of sucrose = 342.29 g/mol
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