Aspirin, C₉H₆O₄, is prepared by reacting salicylic acid, C₇H₆O₃, with acetic anhydride, C₄H₆O₃, in the reaction: 2C₇H₆O₃ + C₄H₆O₃ → 2C₉H₆O₄ + H₂O A student is told to prepare 22.0 g of aspirin. He is also told that he should use a 50.0% excess of acetic anhydride and expect to get a 64.0% yield in the reaction. How many grams of salicylic acid, C₇H₆O₃, should he use? And how many grams of acetic anhydride, C₄H₆O₃, should he use?
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.
Aspirin, C₉H₆O₄, is prepared by reacting salicylic acid, C₇H₆O₃, with acetic anhydride, C₄H₆O₃, in the reaction:
2C₇H₆O₃ + C₄H₆O₃ → 2C₉H₆O₄ + H₂O
A student is told to prepare 22.0 g of aspirin. He is also told that he should use a 50.0% excess of acetic anhydride and expect to get a 64.0% yield in the reaction.
How many grams of salicylic acid, C₇H₆O₃, should he use?
And how many grams of acetic anhydride, C₄H₆O₃, should he use?
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