Exothermic reactions: Releasing heat

In an exothermic reaction, heat is given off (released) when you go from reactants to products. The reaction between oxygen and methane as you light a gas stove (from the earlier section “Reactants and Products: Reading Chemical Equations”) is a good example of an exothermic reaction.

Even though the reaction gives off heat, you do have to put in a little energy — the activation energy — to get the reaction going. You have to ignite the methane coming out of the burners with a match, lighter, pilot light, or built-in electric igniter.

Imagine that the hypothetical reaction A-B + C → C-A + B is exothermic. The reactants start off at a higher energy state than the products, so energy is released in going from reactants to products. Figure 1.1 shows an energy diagram of this reaction.

In the figure, Ea is the activation energy for the reaction. we show the collision of C and A-B with the breaking of the A-B bond and the forming of the C-A bond at the top of an activation-energy hill. This grouping of reactants at the top of the activationenergy hill is sometimes called the transition state of the reaction.

This transition state shows what bonds are being broken and what bonds are being made. As I show in Figure 1.1, the difference in the energy level of the reactants and the energy level of the products is the amount of energy (heat) that is released in the reaction.

Figure 1.1: Exothermic reaction of A-B + C → C-A + B.

مواضيع ذات صلة

Spontaneity: Free Energy and Temperature

Determining ΔG⁰ from Standard Free Energy of Formation

Gibbs Free Energy

Entropy Changes in the Surroundings

Standard Entropy Change of a Reaction, ΔS⁰

Standard Molar Entropy, So

The Boltzmann equation

Qualitative Estimates of Entropy Change

Entropy and the Second Law of Thermodynamics

Thermodynamics

Effect of Changes in Temperature

Effect of Catalysts