2. A student mixed 50.00 mL of 1.00 M HCl at 20.5 °C with 50.00 mL of 1.00 M NH3 at 20.5 °C. After mixing, the temperature rose to 26.6 °C. The calorimeter constant had been determined to be 18.0 J/°C. Assume the density and specific heat capacity of the solution are the same as water, 1.00 g mL-¹ and 4.18 J g-¹ °C-¹, respectively. a) b) Calculate the enthalpy of neutralization in kJ per mole NH3 consumed. Is this reaction endothermic or exothermic?

2. A student mixed 50.00 mL of 1.00 M HCl at 20.5 °C with 50.00 mL of 1.00 M NH3 at 20.5 °C. After mixing, the temperature rose to 26.6 °C. The calorimeter constant had been determined to be 18.0 J/°C. Assume the density and specific heat capacity of the solution are the same as water, 1.00 g mL-¹ and 4.18 J g-¹ °C-¹, respectively. a) b) Calculate the enthalpy of neutralization in kJ per mole NH3 consumed. Is this reaction endothermic or exothermic?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...

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