A coffee cup calorimeter with a heat capacity of 6.00 J/∘6.00 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL50.0 mL solution of 0.330 M AgNO30.330 M AgNO3 was mixed with 50.0 mL50.0 mL of 0.420 M KI.0.420 M KI. After mixing, the temperature was observed to increase by 4.34∘C.4.34∘C. Calculate the enthalpy of reaction, Δ?rxn,ΔHrxn, per mole of precipitate formed (AgI).(AgI). Assume the specific heat of the product solution is 4.15 J / (g⋅∘C)4.15 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL.1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3AgNO3 and KI.KI. moles of precipitate formed from AgNO3:AgNO3: mol moles of precipitate formed from KI:KI: mol Calculate the heat change experienced by the calorimeter contents, ?contents.qcontents. ?contents=qcontents= J Calculate the heat change expierenced by the calorimeter contents, ?cal.qcal. ?cal=qcal= J Calculate the heat change produced by the solution process, ?solution.qsolution. ?solution=qsolution= J Calulate Δ?solutionΔHsolution for one mole of precipitate formed. Δ?solution=
A coffee cup calorimeter with a heat capacity of 6.00 J/∘6.00 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL50.0 mL solution of 0.330 M AgNO30.330 M AgNO3 was mixed with 50.0 mL50.0 mL of 0.420 M KI.0.420 M KI. After mixing, the temperature was observed to increase by 4.34∘C.4.34∘C. Calculate the enthalpy of reaction, Δ?rxn,ΔHrxn, per mole of precipitate formed (AgI).(AgI). Assume the specific heat of the product solution is 4.15 J / (g⋅∘C)4.15 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL.1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3AgNO3 and KI.KI. moles of precipitate formed from AgNO3:AgNO3: mol moles of precipitate formed from KI:KI: mol Calculate the heat change experienced by the calorimeter contents, ?contents.qcontents. ?contents=qcontents= J Calculate the heat change expierenced by the calorimeter contents, ?cal.qcal. ?cal=qcal= J Calculate the heat change produced by the solution process, ?solution.qsolution. ?solution=qsolution= J Calulate Δ?solutionΔHsolution for one mole of precipitate formed. Δ?solution=
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.6: Calorimetry
Problem 2RC: If, in the experiment described in the previous question, some energy as heat is transferred from...
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Question
A coffee cup calorimeter with a heat capacity of 6.00 J/∘6.00 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL50.0 mL solution of 0.330 M AgNO30.330 M AgNO3 was mixed with 50.0 mL50.0 mL of 0.420 M KI.0.420 M KI. After mixing, the temperature was observed to increase by 4.34∘C.4.34∘C. Calculate the enthalpy of reaction, Δ?rxn,ΔHrxn, per mole of precipitate formed (AgI).(AgI). Assume the specific heat of the product solution is 4.15 J / (g⋅∘C)4.15 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL.1.00 g/mL.
Calculate the theoretical moles of precipitate formed from AgNO3AgNO3 and KI.KI.
moles of precipitate formed from AgNO3:AgNO3:
mol
moles of precipitate formed from KI:KI:
mol
Calculate the heat change experienced by the calorimeter contents, ?contents.qcontents.
?contents=qcontents=
J
Calculate the heat change expierenced by the calorimeter contents, ?cal.qcal.
?cal=qcal=
J
Calculate the heat change produced by the solution process, ?solution.qsolution.
?solution=qsolution=
J
Calulate Δ?solutionΔHsolution for one mole of precipitate formed.
Δ?solution=
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