A coffee cup calorimeter with a heat capacity of 4.90 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AgNO3 was mixed with 50.0 mL of 0.480 M KCl. After mixing, the temperature was observed to increase by 2.80∘C.Calculate the enthalpy of reaction, Δ?rxn, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.17 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 AgNO3 and KCl. Calculate the heat change experienced by the calorimeter contents, ?contents. Calculate the heat change experienced by the calorimeter, ?cal. Calculate the heat change produced by the solution process, ?solution. Calulate Δ?solution for one mole of precipitate formed.
A coffee cup calorimeter with a heat capacity of 4.90 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AgNO3 was mixed with 50.0 mL of 0.480 M KCl. After mixing, the temperature was observed to increase by 2.80∘C.Calculate the enthalpy of reaction, Δ?rxn, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.17 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 AgNO3 and KCl.
Calculate the heat change experienced by the calorimeter contents, ?contents.
Calculate the heat change experienced by the calorimeter, ?cal.
Calculate the heat change produced by the solution process, ?solution.
Calulate Δ?solution for one mole of precipitate formed.
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