The combustion of one mole of sucrose (C12H22O11) releases 5.65 × 103 kJ of heat. (a) Write a balanced equation for the combustion of sucrose. Also, provide the ΔHrxn next to the balanced equation. The balanced chemical equation and its corresponding ΔH value are called a thermochemical equation. Determine whether this reaction is exothermic or endothermic. (b) Redefine ΔHrxn with respect to each reactant and product in the reaction. One example is shown for you. ΔHrxn = -5.65 x 103 kJ = -5.65 x 103 kJ = 1 mol “reaction” 1 mol C12H22O11 (c) If 5.00 moles of CO2 were produced, what is the heat for the reaction, qrxn, in kJ? (d)What mass of sucrose must be burned to produce 1.00 × 103 kJ of heat?
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 combustion of one mole of sucrose (C12H22O11) releases 5.65 × 103 kJ of heat.
(a) Write a balanced equation for the combustion of sucrose. Also, provide the ΔHrxn next to the balanced equation. The balanced chemical equation and its corresponding ΔH value are called a thermochemical equation.
Determine whether this reaction is exothermic or endothermic.
(b) Redefine ΔHrxn with respect to each reactant and product in the reaction. One example is shown for you.
ΔHrxn = -5.65 x 103 kJ = -5.65 x 103 kJ =
1 mol “reaction” 1 mol C12H22O11
(c) If 5.00 moles of CO2 were produced, what is the heat for the reaction, qrxn, in kJ?
(d)What mass of sucrose must be burned to produce 1.00 × 103 kJ of heat?
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