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

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

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction,
3
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 HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
ΔΗ -
kJ/mol

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