A 115.0-g sample of a metal at 165.0 °C is added to 265.0 g of ethylene glycol (specific heat = 2.43 J/g °C) in a calorimeter at 25.8 °C. The temperature of the ethylene glycol rises to 41.5 °C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the ethylene glycol.

A 115.0-g sample of a metal at 165.0 °C is added to 265.0 g of ethylene glycol (specific heat = 2.43 J/g °C) in a calorimeter at 25.8 °C. The temperature of the ethylene glycol rises to 41.5 °C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the ethylene glycol.

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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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.

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