In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCI are mixed. Both solutions were originally at 24.0°C. After the reaction, the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ- kJ/mol

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCI are mixed. Both solutions were originally at 24.0°C. After the reaction, the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ- kJ/mol

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 59E: In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed to yield...

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