Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 48.7 g of KNO, is dissolved in 259 g of water at 23.00 °C. H,0 KNO, (s) K*(aq) + NO, (aq) The temperature of the resulting solution decreases to 18.10 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g · °C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? 4soln = kJ What is the enthalpy of the reaction? ΔΗΧ kJ/mol rxn

Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 48.7 g of KNO, is dissolved in 259 g of water at 23.00 °C. H,0 KNO, (s) K*(aq) + NO, (aq) The temperature of the resulting solution decreases to 18.10 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g · °C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? 4soln = kJ What is the enthalpy of the reaction? ΔΗΧ kJ/mol rxn

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 5.61QE: When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases...

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