1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? c) Which of the reactants is the limiting reagent? Justify your answer.
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.
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2.
a) Write a balanced chemical equation for the reaction.
b) What mass of acetic acid is in the aqueous solution?
c) Which of the reactants is the limiting reagent? Justify your answer.
d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction?
e) What is the theoretical yield (in grams) of carbon dioxide from this reaction?
f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?
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1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2.
d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction?
e) What is the theoretical yield (in grams) of carbon dioxide from this reaction?
f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?
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