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Chapter 6: Problem 14

How is average bond strength related to relative potential energies of the reactants and the products?

Short Answer

Expert verified
The average bond strength in a chemical reaction is related to the relative potential energies of the reactants and products, such that if the average bond strength increases during the reaction, the potential energy of the products is lower than that of the reactants. Conversely, if the average bond strength decreases, the potential energy of the products is higher than that of the reactants. This is because stronger bonds are more stable and require more energy to break, leading to a decrease in potential energy when bond strength increases.

Step by step solution

01

Understand the terms potential energy and bond strength

Potential energy is the energy stored in a substance due to its chemical composition and the arrangement of its atoms. In a chemical reaction, potential energy may change as bonds between atoms are formed or broken. Bond strength, also known as bond energy, is a measure of the amount of energy required to break a chemical bond between two atoms. It is an indication of the stability of a chemical bond or a molecule. Stronger bonds have higher bond strengths, while weaker bonds have lower bond strengths.
02

Know the relationship between potential energy and bond strength

In a chemical reaction, the difference in potential energy between the reactants and the products is related to the bond strengths of the molecules involved. The potential energy of a system decreases when the bond strength of the molecules increases, as stronger bonds are more stable and require more energy to break.
03

Determine the reactants and products in a chemical reaction

For a given chemical reaction, identify the reactants and products involved. This will help us analyze the changes in potential energy and bond strengths between the initial state (reactants) and the final state (products).
04

Analyze the difference in bond strength between reactants and products

Calculate the differences in bond strength for each bond between the reactants and the products. This will help us to determine the overall change in bond strength during the chemical reaction.
05

Establish the relationship between average bond strength and potential energy changes

To find out the relationship between average bond strength and the relative potential energies of the reactants and products, we need to compare the changes in bond strength with the changes in potential energy. If the average bond strength increases during the reaction, the potential energy of the products should be lower than the potential energy of the reactants. Conversely, if the average bond strength decreases during the reaction, the potential energy of the products should be higher than the potential energy of the reactants. In conclusion, the average bond strength of the molecules in a chemical reaction is related to the relative potential energies of the reactants and the products. If the average bond strength increases during a chemical reaction, the potential energy of the products is lower than the potential energy of the reactants. If the average bond strength decreases during the reaction, the potential energy of the products is higher than the potential energy of the reactants.

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Most popular questions from this chapter

For each of the following situations a-c, use choices i-iii to complete the statement: "The final temperature of the water should be.." i. between \(50^{\circ} \mathrm{C}\) and \(90^{\circ} \mathrm{C}\) . ii. \(50^{\circ} \mathrm{C}\) . iii. between \(10^{\circ} \mathrm{C}\) and \(50^{\circ} \mathrm{C}\) . a. 100.0 -g sample of water at \(90^{\circ} \mathrm{C}\) is added to a 100.0 -g sample of water at \(10^{\circ} \mathrm{C}\) . b. A 100.0 -g sample of water at \(90^{\circ} \mathrm{C}\) is added to a \(500.0 . \mathrm{g}\) sample of water at \(10^{\circ} \mathrm{C} .\) c. You have a Styrofoam cup with 50.0 \(\mathrm{g}\) of water at \(10^{\circ} \mathrm{C}\) . You add a 50.0 -g iron ball at \(90^{\circ} \mathrm{C}\) to the water.

Are the following processes exothermic or endothermic? a. When solid \(\mathrm{KBr}\) is dissolved in water, the solution gets colder. b. Natural gas \(\left(\mathrm{CH}_{4}\right)\) is burned in a furnace. c. When concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is added to water, the solution gets very hot. d. Water is boiled in a teakettle.

Calculate \(w\) and \(\Delta E\) when 1 mole of a liquid is vaporized at its boiling point \(\left(80 .^{\circ} \mathrm{C}\right)\) and 1.00 atm pressure. \(\Delta H_{\text { vap }}\) for the liquid is 30.7 \(\mathrm{kJ} / \mathrm{mol}\) at \(80 .^{\circ} \mathrm{C} .\)

Given: $$ \begin{array}{ll}{2 \mathrm{Cu}_{2} \mathrm{O}(s)+\mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{CuO}(s)} & {\Delta H^{\circ}=-288 \mathrm{kJ}} \\\ {\mathrm{Cu}_{2} \mathrm{O}(s) \longrightarrow \mathrm{CuO}(s)+\mathrm{Cu}(s)} & {\Delta H^{\circ}=11 \mathrm{kJ}}\end{array} $$ Calculate the standard enthalpy of formation \(\left(\Delta H_{f}^{\circ}\right)\) for \(\mathrm{CuO}(s) .\)

The specific heat capacity of silver is 0.24 \(\mathrm{J} /^{\circ} \mathrm{C} \cdot \mathrm{g}\) a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 \(\mathrm{K}\) to 298 \(\mathrm{K}\) . b. Calculate the energy required to raise the temperature of 1.0 mole of \(\mathrm{Ag}\) by \(1.0^{\circ} \mathrm{C}\) (called the molar heat capacity of silver). c. It takes 1.25 \(\mathrm{kJ}\) of energy to heat a sample of pure silver from \(12.0^{\circ} \mathrm{C}\) to \(15.2^{\circ} \mathrm{C}\) . Calculate the mass of the sample of silver.
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