A coffee cup calorimeter with a heat capacity of 7.40 JrC was used to measure the change in enthalpy of a precipitationreaction. A 50.0 mL solution of 0.360 M AGNO, was mixed with 50.0 mL of 0.310 M KBr. After mixing, thetemperature was observed to increase by 3.04 °C. Calculate the enthalpy of reaction, AHan, per mole of precipitateformed (AgBr). Assume the specific heat of the product solution is 4.11 J/ (g C) and that the density of both thereactant solutions is 1.00 g/mL.Calculate the theoretical moles of precipitate formed from AgNO, and KBr.theoretical moles of precipitate formed from AgNO,:molestheoretical moles of precipitate formed from KBr:molesCalculate the heat change experienced by the calorimeter contents, qontents - theoretical moles of precipitate formed from KBr:molesCalculate the heat change experienced by the calorimeter contents, qontents-contents =Calculate the heat change expierenced by the calorimeter contents, qcal-Ical =JCalculate the heat change produced by the solution process, 4solution·9solution =Calulate AHolution for one mole of precipitate formed.AHsolution =kJ/mole

Answered: Image /qna-images/answer/68147ab5-3dab-4573-90d0-8828363be0a0.jpg

Answered: J contents = Calculate the heat change…

J contents = Calculate the heat change expierenced by the calorimeter contents, qcal- J 9cal = Calculate the heat change produced by the solution process, Isolution · J 9solution

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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Concept explainers

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

A coffee cup calorimeter with a heat capacity of 7.40 JrC was used to measure the change in enthalpy of a precipitation
reaction. A 50.0 mL solution of 0.360 M AGNO, was mixed with 50.0 mL of 0.310 M KBr. After mixing, the
temperature was observed to increase by 3.04 °C. Calculate the enthalpy of reaction, AHan, per mole of precipitate
formed (AgBr). Assume the specific heat of the product solution is 4.11 J/ (g C) and that the density of both the
reactant solutions is 1.00 g/mL.
Calculate the theoretical moles of precipitate formed from AgNO, and KBr.
theoretical moles of precipitate formed from AgNO,:
moles
theoretical moles of precipitate formed from KBr:
moles
Calculate the heat change experienced by the calorimeter contents, qontents -

theoretical moles of precipitate formed from KBr:
moles
Calculate the heat change experienced by the calorimeter contents, qontents-
contents =
Calculate the heat change expierenced by the calorimeter contents, qcal-
Ical =
J
Calculate the heat change produced by the solution process, 4solution·
9solution =
Calulate AHolution for one mole of precipitate formed.
AHsolution =
kJ/mole

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