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?
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 104AE
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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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