Potassium nitrate, KNO3KNO3, has a molar mass of 101.1101.1 g/mol. In a constant-pressure calorimeter, 23.223.2 g of KNO3KNO3 is dissolved in 341341 g of water at 23.00 °C23.00 °C. KNO3(s)−→−−H2OK+(aq)+NO−3(aq)KNO3(s)→H2OK+(aq)+NO3−(aq) The temperature of the resulting solution decreases to 17.50 °C17.50 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g·°C)4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? ?soln=qsoln= kJkJ What is the enthalpy of the reaction? Δ?rxn=ΔHrxn= kJ/mol
Potassium nitrate, KNO3KNO3, has a molar mass of 101.1101.1 g/mol. In a constant-pressure calorimeter, 23.223.2 g of KNO3KNO3 is dissolved in 341341 g of water at 23.00 °C23.00 °C. KNO3(s)−→−−H2OK+(aq)+NO−3(aq)KNO3(s)→H2OK+(aq)+NO3−(aq) The temperature of the resulting solution decreases to 17.50 °C17.50 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g·°C)4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? ?soln=qsoln= kJkJ What is the enthalpy of the reaction? Δ?rxn=ΔHrxn= 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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Potassium nitrate, KNO3KNO3, has a molar mass of 101.1101.1 g/mol. In a constant-pressure calorimeter, 23.223.2 g of KNO3KNO3 is dissolved in 341341 g of water at 23.00 °C23.00 °C.
KNO3(s)−→−−H2OK+(aq)+NO−3(aq)KNO3(s)→H2OK+(aq)+NO3−(aq)
The temperature of the resulting solution decreases to 17.50 °C17.50 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g·°C)4.184 J/(g·°C), and that there is negligible heat loss to the surroundings.
How much heat was released by the solution?
?soln=qsoln=
kJkJ
What is the enthalpy of the reaction?
Δ?rxn=ΔHrxn=
kJ/mol
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