**Question 5: Determining the True Statement About Enthalpy**The question focuses on identifying the correct statement related to the concept of enthalpy in thermodynamics.**Provided Statements:**1. The enthalpy change for a reaction is independent of the state of the reactants and products.2. Enthalpy is a state function.3. \( H \) is the value of \( q \) measured under conditions of constant volume.4. The enthalpy change of a reaction is the reciprocal of the \( \Delta H \) of the reverse reaction.**Explanation:**- **State Function:** A property that depends only on the current state of the system, not on the path taken to reach that state.- **Enthalpy (\( H \)):** A thermodynamic quantity equivalent to the total heat content of a system, defined as \( H = U + PV \), where \( U \) is the internal energy, \( P \) is pressure, and \( V \) is volume.- Enthalpy changes in reactions typically occur at constant pressure, not constant volume.- The enthalpy change (\( \Delta H \)) of a reverse reaction is equal in magnitude but opposite in sign, not reciprocal.Understanding these concepts is crucial for analyzing thermodynamic processes accurately.

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5) Which one of the following statements is true? The enthalpy change for a for a reaction is independent of the state of the reactants and products. Enthalpy is a state function. H is the value of q measured under conditions of constant volume. The enthalpy change of a reaction is the reciprocal of the AH of the reverse reaction. Page 2 of 8

5) Which one of the following statements is true? The enthalpy change for a for a reaction is independent of the state of the reactants and products. Enthalpy is a state function. H is the value of q measured under conditions of constant volume. The enthalpy change of a reaction is the reciprocal of the AH of the reverse reaction. Page 2 of 8

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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