Using a coffee cup calorimeter, 3.15 g of ammonium chloride, NH4Cl is added 100.0 g of water at 25.0 °C, the temperature of the water drops down to 21.9 °C as the ammonium chloride dissolves. Assume that mass of the solution is equal to the mass of the ammonium chloride and the mass of the water. Also assume that the specific heat of the solution is 4.18 J/g*K. Calculate the enthalpy change (AH rxn) in kJ/mol of ammonium chloride for the energy change that accompanies this dissolving process. Find AH of: NH4CI(s) -->NH4*(aq) +Cl(aq) (The enthalpy of dissolving) A

Using a coffee cup calorimeter, 3.15 g of ammonium chloride, NH4Cl is added 100.0 g of water at 25.0 °C, the temperature of the water drops down to 21.9 °C as the ammonium chloride dissolves. Assume that mass of the solution is equal to the mass of the ammonium chloride and the mass of the water. Also assume that the specific heat of the solution is 4.18 J/gK. Calculate the enthalpy change (AH rxn) in kJ/mol of ammonium chloride for the energy change that accompanies this dissolving process. Find AH of: NH4CI(s) -->NH4(aq) +Cl(aq) (The enthalpy of dissolving) A

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 66E: In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both...

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