I did a lab in which I dissolved sodium bicarbonate and sodium acetate in water, using a simple styrofoam cup as a calorimeter. For sodium bicarbonate, the temperature decreased from 20.8 degrees Celsius to 16.6 degrees Celsius. For sodium acetate, the temperature decreased from 18.4 degrees Celsius to 17.5 degrees Celsius. I used 150 mL of water to dissolve sodium bicarbonate, and 32.5 mL of water to dissolve sodium acetate. I used 15 grams of sodium bicarbonate and 3.25 grams of sodium acetate. I calculated that -2.64 kJ was released in the reaction for sodium bicarbonate, and -0.122 kJ was released in the reaction for sodium acetate. I also calculated that 0.18 moles of sodium bicarbonate were used and 0.0396 moles of sodium acetate was used. I then got -14.67 kJ/mol as the molar heat of solution for sodium bicarbonate, and -3.08 kJ/mol for the molar heat of solution for sodium acetate. However, when I calculate the percent errors, I am getting numbers of over 100. Did I do something wrong here?
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.
I did a lab in which I dissolved sodium bicarbonate and sodium acetate in water, using a simple styrofoam cup as a calorimeter. For sodium bicarbonate, the temperature decreased from 20.8 degrees Celsius to 16.6 degrees Celsius. For sodium acetate, the temperature decreased from 18.4 degrees Celsius to 17.5 degrees Celsius. I used 150 mL of water to dissolve sodium bicarbonate, and 32.5 mL of water to dissolve sodium acetate. I used 15 grams of sodium bicarbonate and 3.25 grams of sodium acetate. I calculated that -2.64 kJ was released in the reaction for sodium bicarbonate, and -0.122 kJ was released in the reaction for sodium acetate. I also calculated that 0.18 moles of sodium bicarbonate were used and 0.0396 moles of sodium acetate was used. I then got -14.67 kJ/mol as the molar heat of solution for sodium bicarbonate, and -3.08 kJ/mol for the molar heat of solution for sodium acetate. However, when I calculate the percent errors, I am getting numbers of over 100. Did I do something wrong here?
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