50.0 g of NH4Cl(s) (53.49 g mol–1) is dissolved in 200.0 mL of H2O in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The final temperature is 7.13°C. The density of water is 1.00 g cm–3. The specific heat of the solution is 4.184 J g–1 °C–1. What is the heat of the dissolution reaction? What is the energy change of the solution?
50.0 g of NH4Cl(s) (53.49 g mol–1) is dissolved in 200.0 mL of H2O in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The final temperature is 7.13°C. The density of water is 1.00 g cm–3. The specific heat of the solution is 4.184 J g–1 °C–1. What is the heat of the dissolution reaction? What is the energy change of the solution?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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50.0 g of NH4Cl(s) (53.49 g mol–1) is dissolved in 200.0 mL of H2O in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The final temperature is 7.13°C. The density of water is 1.00 g cm–3. The specific heat of the solution is 4.184 J g–1 °C–1.
What is the heat of the dissolution reaction?
What is the energy change of the solution?
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