In the design of an experiment to the measure the heat change of a chemical reaction in an aqueous solution we make the following assumptions: (1) we assume our calorimeter is a perfect insulator and no heat is transfered to the surroundings and (2) we assume that negligible heat is absorbed by the calorimeter. We could write the following equation representing the relationship between the heat changes in our system. qsystem = qcalorimeter + qreaction + qsolution Considering the design of the experiment, in the above equation which heat changes would we assume are equal to zero?
In the design of an experiment to the measure the heat change of a chemical reaction in an aqueous solution we make the following assumptions: (1) we assume our calorimeter is a perfect insulator and no heat is transfered to the surroundings and (2) we assume that negligible heat is absorbed by the calorimeter. We could write the following equation representing the relationship between the heat changes in our system. qsystem = qcalorimeter + qreaction + qsolution Considering the design of the experiment, in the above equation which heat changes would we assume are equal to zero?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
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In the design of an experiment to the measure the heat change of a
qsystem = qcalorimeter + qreaction + qsolution
Considering the design of the experiment, in the above equation which heat changes would we assume are equal to zero?
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