Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question

A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 ∘C25.00 ∘C to 23.87 ∘C23.87 ∘C . Calculate the enthalpy of solution, Δ?solnΔHsoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.13 J/(g⋅∘C4.13 J/(g⋅∘C ) and the heat capacity of the calorimeter is 3.30 J/ ∘C3.30 J/ ∘C .

Calculate the heat change experienced by the calorimeter contents, ?contentsqcontents .

?contents=qcontents=
 
JJ
Calculate the heat change experienced by the calorimeter, ?calqcal .
?cal=qcal=
 
JJ
Calculate the heat change produced by the solution process, ?solnqsoln .
?soln=qsoln=
 
JJ
Calculate Δ?solnΔHsoln , the enthalpy of solution for one mole of solid in kilojoules per mole.
Δ?soln=ΔHsoln=
 
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