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Chapter 9: Problem 82

Why must the structures of the reactants and products be known in order to estimate the enthalpy change of a reaction from bond energies?

Short Answer

Expert verified
Answer: Knowing the structures of reactants and products is essential for estimating the enthalpy change of a reaction using bond energies because it allows us to identify all the bonds involved in the reaction and their corresponding bond energies. This information is crucial for accurately calculating the sum of bond energies for both reactants and products, which in turn is used to determine the enthalpy change and whether the reaction is endothermic or exothermic. Without this knowledge, the estimation of enthalpy change would be inaccurate.

Step by step solution

01

Define bond energy and enthalpy change

Bond energy is the amount of energy needed to break a particular chemical bond in one mole of gaseous molecules. Enthalpy change (螖H) refers to the heat absorbed or released during a chemical reaction. It can be used to determine whether the reaction is endothermic (absorbing energy) or exothermic (releasing energy).
02

Understand the relationship between bond energies and enthalpy change

To calculate the enthalpy change in a chemical reaction using bond energies, we use the following formula: 螖H = 危 (bond energies of reactants) - 危 (bond energies of products) This is essentially the difference between the energy required to break all the bonds in the reactants and the energy released upon the formation of all the bonds in the products.
03

Significance of knowing structures of reactants and products

In order to estimate the enthalpy change using bond energies, we must know the structures of both reactants (the molecules before the reaction) and products (the molecules after the reaction). Knowing the structures will allow us to identify all the bonds involved in the reaction and their corresponding bond energies. Without this information, it would be impossible to calculate the sum of bond energies for both reactants and products accurately, consequently making the estimation of enthalpy change inaccurate.
04

Example of importance of knowing structures

For example, let's consider the following reaction: H2(g) + Cl2(g) -> 2 HCl(g) Here, we know the structures of reactants H2 and Cl2 as diatomic molecules, and the structure of the product HCl as a simple molecule. We can use their bond energies to estimate the enthalpy change of this reaction: Bond energy of H-H (in H2) = 436 kJ/mol Bond energy of Cl-Cl (in Cl2) = 242 kJ/mol Bond energy of H-Cl (in HCl) = 431 kJ/mol 螖H = (436 + 242) - 2(431) = -183 kJ/mol In this case, the reaction is exothermic as the enthalpy change is negative. Therefore, knowing the structures of reactants and products is essential for determining the enthalpy change of a reaction using bond energies accurately.

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Most popular questions from this chapter

The destruction of the ozone layer by chlorofluorocarbons (CFCs) can be described by the following reactions: $$\begin{aligned}\mathrm{ClO}(g)+\mathrm{O}_{3}(g) & \rightarrow \mathrm{Cl}(g)+2 \mathrm{O}_{2}(g) & \Delta H_{\mathrm{rxn}}^{\circ} &=-29.90 \mathrm{kJ} \\\2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) & & \Delta H_{\mathrm{rxn}}^{\circ} &=+24.18 \mathrm{kJ}\end{aligned}$$ Use the preceding \(\Delta H_{\mathrm{rxn}}^{\circ}\) values to determine the value of the standard heat of reaction for this reaction: $$\mathrm{Cl}(g)+\mathrm{O}_{3}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=?$$

Which of the following processes are exothermic, and which are endothermic? a. Ice cubes solidify in the freezer. b. Ice cubes in a frost-free freezer slowly lose mass. c. Dew forms on a lawn overnight.

What is meant by an entbalpy change?

Explain what is meant by a state function.

Why must the stoichiometry of a reaction be known in order to estimate the enthalpy change from bond energies?
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