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10 Nov 2019
A coffee cup calorimeter with a heat capacity of 3.60 J/degree C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.340 M AgNO3 was mixed with 500 mL of 0.410 M KCI. After mixing, the temperature was observed to increase by 2.68 degree C. Calculate the enthalpy of reaction, deltaHrmx, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.13 J/(g. degree C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3 (left) and KCl (right). Number ____________ moles Number moles Calculate the heat change experienced by the calorimeter contents, qcontents. Number ________________ J Calculate the heat change produced by the solution process, qsolution __________ Using the mole values calculated above, calculate deltaHsolution for one mole of precipitate formed. Number ______ KJ/mol
A coffee cup calorimeter with a heat capacity of 3.60 J/degree C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.340 M AgNO3 was mixed with 500 mL of 0.410 M KCI. After mixing, the temperature was observed to increase by 2.68 degree C. Calculate the enthalpy of reaction, deltaHrmx, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.13 J/(g. degree C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3 (left) and KCl (right). Number ____________ moles Number moles Calculate the heat change experienced by the calorimeter contents, qcontents. Number ________________ J Calculate the heat change produced by the solution process, qsolution __________ Using the mole values calculated above, calculate deltaHsolution for one mole of precipitate formed. Number ______ KJ/mol
Sixta KovacekLv2
23 Oct 2019