Adding 4.88 g of NH4NO3(s) to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 19.0 °C to 16.7 °C. Calculate the enthalpy change for dissolving NH4NO3(s) in water in kJ/mol. Assume the solution (whose mass is 144.9 g) has a specific heat capacity of 4.2 J/g K. (Cold packs take advantage of the fact that dissolving ammonium nitrate in water is an endothermic process.) A cold pack uses the endothermic enthalpy of a solution of ammonium nitrate. Enthalpy change= kJ/mol

Adding 4.88 g of NH4NO3(s) to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 19.0 °C to 16.7 °C. Calculate the enthalpy change for dissolving NH4NO3(s) in water in kJ/mol. Assume the solution (whose mass is 144.9 g) has a specific heat capacity of 4.2 J/g K. (Cold packs take advantage of the fact that dissolving ammonium nitrate in water is an endothermic process.) A cold pack uses the endothermic enthalpy of a solution of ammonium nitrate. Enthalpy change= kJ/mol

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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