   Chapter 17, Problem 3ALQ

Chapter
Section
Textbook Problem

# Gas A2 reacts with gas B2 to form gas AB at a constant temperature. The bond energy of AB is much greater than that of either reactant. What can be said about the sign of ∆H? ∆SSurr? ∆S? Explain how potential energy changes for this process. Explain how random kinetic energy changes during the process.

Interpretation Introduction

Interpretation: A gas A2 is given to react with a gas B2 to form a gas AB at a constant temperature. The bond energy of AB is stated to be greater than each of the given reactants. A comment on the sign of ΔS,ΔH and ΔSsurr . The potential energy changes and the change in the random kinetic energy is to be explained.

Concept introduction: The atoms of the product species are held by stronger bonds as compared to the atoms in the reactants. Hence, the entropy of products is considered to be less than the entropy of the reactants.

To determine: A comment on the sign of ΔS,ΔH and ΔSsurr ; the potential energy changes and the change in the random kinetic energy.

Explanation

Explanation

Te stated reaction is,

A2(g)+B2(g)2AB(g)

The bond energy of AB is stated to be greater than each of the given reactants. Hence, the products will have a higher potential energy than that of the reactants. The reaction is hence an endothermic reaction. The ΔH of an endothermic reaction is positive.

The energy is gained by the system from the surroundings in the given system. Therefore,

ΔSsurr=Negative

The atoms of the product species are held by stronger bonds as compared to the atoms in the reactants

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