A 8.33 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. a. What is the total mass inside the calorimeter in grams? b. What is the change in temperature, in °C, inside the calorimeter? c. Was the dissolution process endothermic or exothermic? d. What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g･ °C. e. What is the total heat for the dissolution reaction of the 8.33 g of salt? f. What quantity in moles of the unknown salt were used in the reaction? g. What is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
A 8.33 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. a. What is the total mass inside the calorimeter in grams? b. What is the change in temperature, in °C, inside the calorimeter? c. Was the dissolution process endothermic or exothermic? d. What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g･ °C. e. What is the total heat for the dissolution reaction of the 8.33 g of salt? f. What quantity in moles of the unknown salt were used in the reaction? g. What is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
Question
4. A 8.33 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C.
a. What is the total mass inside the calorimeter in grams?
b. What is the change in temperature, in °C, inside the calorimeter?
c. Was the dissolution process endothermic or exothermic?
d. What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g･ °C.
e. What is the total heat for the dissolution reaction of the 8.33 g of salt?
f. What quantity in moles of the unknown salt were used in the reaction?
g. What is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
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