When 50.0 mL of 0.100 AgNO3 and 50.0 mL of 0.100 HCl are mixed in a constant-pressure M M calorimeter, the temperature of the mixture increases from 22.3°C to 23.1°C. The temperature increase is caused by the following reaction: + HCl(aq) AgCl(s) + HNO3(aq) = ? ΔH Calculate for this reaction in kJ/mol AgNO3, assuming that the combined solution has a mass of 100.0 ΔH g and a specific heat of 4.18 J/g·°C. When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee cup calorimeter, the temperature rises from 21.6°C to 37.8°C. Calculate (in kJ/mol NaOH) for the solution process: ΔH NaOH(s) Na+(aq) + OH-(aq) = ? ΔH Assume the specific heat of the solution is the same as pure water. NOTE: Mass of solution includes solute AND solvent. When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0°C to 16.9°C. Calculate the (in kJ/mol NH4NO3) for the solution ΔH process: NH4NO3 (s) NH4+ (aq) + NO3-(aq) = ? ΔH Assume that the specific heat of the solution is the same as that of pure POTENTIAL ENERGY DIAGRAMS (ENTHALPY OF A REACTION) Diagrams relative energies of reactants and products in a reaction. The difference between the levels represents the change in enthalpy (ΔH). Exothermic energy is released
When 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed in a constant-pressure calorimeter, the temperature of the mixture increases from 22.3°C to 23.1°C. The temperature increase is caused by the following reaction: + HCl(aq) AgCl(s) + HNO3(aq) ΔH = ? Calculate ΔH for this reaction in kJ/mol AgNO3, assuming that the combined solution has a mass of 100.0 g and a specific heat of 4.18 J/g·°C. When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee cup calorimeter, the temperature rises from 21.6°C to 37.8°C. Calculate ΔH (in kJ/mol NaOH) for the solution process: NaOH(s) Na+(aq) + OH-(aq) ΔH = ? Assume the specific heat of the solution is the same as pure water. NOTE: Mass of solution includes solute AND solvent. When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0°C to 16.9°C. Calculate the ΔH (in kJ/mol NH4NO3) for the solution process: NH4NO3 (s) NH4+ (aq) + NO3-(aq) ΔH = ? Assume that the specific heat of the solution is the same as that of pure POTENTIAL ENERGY DIAGRAMS (ENTHALPY OF A REACTION) Diagrams relative energies of reactants and products in a reaction. The difference between the levels represents the change in enthalpy (ΔH). Exothermic energy is released
unit_5_students_notes_packet.docx