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Chapter 14: Problem 27

Define activation energy. What role does activation energy play in chemical kinetics?

Short Answer

Expert verified
Activation energy is the minimum energy required for a reaction to happen. It plays a vital role in chemical kinetics by influencing the rate of reactions. Higher activation energy results in slower reaction rates, and vice versa. Temperature also plays a role by affecting how many molecules can overcome the activation energy barrier.

Step by step solution

01

Define Activation Energy

Activation energy, often represented as \(E_a\), is the minimum amount of energy that reactants must possess for a chemical reaction to occur. It serves as a barrier to the progress of a reaction. No reaction can occur unless the reactant molecules possess this required amount of energy.
02

Explain Activation Energy鈥檚 Role in Chemical Kinetics

Activation energy plays a key role in chemical kinetics, which deal with the rate of reactions. Higher activation energy implies that fewer molecules will have sufficient energy to react, thus the reaction rate will be slower. Conversely, a lower activation energy means that more molecules can undergo the reaction, leading to a faster reaction rate. Temperature also affects this process. As temperature increases, more molecules possess the necessary energy to exceed the activation energy barrier, hence the reaction rate increases.

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Most popular questions from this chapter

The rate law for the reaction $$ \mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ is given by rate \(=k\left[\mathrm{NH}_{4}^{+}\right]\left[\mathrm{NO}_{2}^{-}\right]\). At \(25^{\circ} \mathrm{C},\) the rate constant is \(3.0 \times 10^{-4} / M \cdot\) s. Calculate the rate of the reaction at this temperature if \(\left[\mathrm{NH}_{4}^{+}\right]=0.26 \mathrm{M}\) and \(\left[\mathrm{NO}_{2}^{-}\right]=0.080 \mathrm{M}\)

A quantity of \(6 \mathrm{~g}\) of granulated \(\mathrm{Zn}\) is added to a solution of \(2 M \mathrm{HCl}\) in a beaker at room temperature. Hydrogen gas is generated. For each of the following changes (at constant volume of the acid) state whether the rate of hydrogen gas evolution will be increased, decreased, or unchanged: (a) \(6 \mathrm{~g}\) of powdered \(\mathrm{Zn}\) is used; \((\mathrm{b}) 4 \mathrm{~g}\) of granulated \(\mathrm{Zn}\) is used; \((\mathrm{c})\) \(2 M\) acetic acid is used instead of \(2 M \mathrm{HCl} ;\) d) temperature is raised to \(40^{\circ} \mathrm{C}\).

Briefly comment on the effect of a catalyst on each of the following: (a) activation energy, (b) reaction mechanism, (c) enthalpy of reaction, (d) rate of forward step, (e) rate of reverse step.

For the reaction $$ \mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g) $$ the frequency factor \(A\) is \(8.7 \times 10^{12} \mathrm{~s}^{-1}\) and the activation energy is \(63 \mathrm{~kJ} / \mathrm{mol}\). What is the rate constant for the reaction at \(75^{\circ} \mathrm{C} ?\)

When methyl phosphate is heated in acid solution, it reacts with water: $$ \mathrm{CH}_{3} \mathrm{OPO}_{3} \mathrm{H}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{CH}_{3} \mathrm{OH}+\mathrm{H}_{3} \mathrm{PO}_{4} $$ If the reaction is carried out in water enriched with \({ }^{18} \mathrm{O}\), the oxygen- 18 isotope is found in the phosphoric acid product but not in the methanol. What does this tell us about the bond-breaking scheme in the reaction?
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