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Chapter 14: Problem 50

What are the characteristics of a catalyst?

Short Answer

Expert verified
A catalyst is a substance that speeds up a chemical reaction without being consumed by the reaction. It can work in either homogeneous or heterogeneous catalysis, providing a lower-energy pathway for the reaction. Crucially, while catalysts speed up the rate of both the forward and reverse reactions, they do not shift the equilibrium of the reaction.

Step by step solution

01

Identifying Characteristics of a Catalyst

Firstly, we can begin by stating that a catalyst is a substance that speeds up a chemical reaction without being consumed by the reaction. This means that a catalyst can be used repeatedly for the same reaction because it does not get used up.
02

Additional Properties

Secondly, it's important to note that catalysts can be in the same phase as the reactants, known as homogeneous catalysis, or in a different phase, known as heterogeneous catalysis. The catalyst changes the mechanism of the reaction, often by providing a lower-energy pathway for the reaction to occur.
03

Role of a Catalyst

Lastly, catalysts do not change the equilibrium of a reaction. They only affect the rate at which the equilibrium is reached. That is, the catalysts speed up the rate of both the forward and reverse reactions equally, allowing the system to reach equilibrium faster but does not shift the position of the equilibrium.

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Most popular questions from this chapter

Consider the zero-order reaction \(\mathrm{A} \longrightarrow\) product. (a) Write the rate law for the reaction. (b) What are the units for the rate constant? (c) Plot the rate of the reaction versus [A].

The following gas-phase reaction was studied at \(290^{\circ} \mathrm{C}\) by observing the change in pressure as a function of time in a constant-volume vessel: $$ \mathrm{ClCO}_{2} \mathrm{CCl}_{3}(g) \longrightarrow 2 \mathrm{COCl}_{2}(g) $$ Determine the order of the reaction and the rate constant based on the following data: $$ \begin{array}{rc} \text { Time }(\mathrm{s}) & \mathrm{P}(\mathrm{mmHg}) \\ \hline 0 & 15.76 \\ 181 & 18.88 \\ 513 & 22.79 \\ 1164 & 27.08 \end{array} $$ where \(P\) is the total pressure.

Radioactive plutonium- \(239\left(t_{\frac{1}{2}}=2.44 \times 10^{5} \mathrm{yr}\right)\) is used in nuclear reactors and atomic bombs. If there are \(5.0 \times 10^{2} \mathrm{~g}\) of the isotope in a small atomic bomb, how long will it take for the substance to decay to \(1.0 \times 10^{2} \mathrm{~g},\) too small an amount for an effective bomb? (Hint: Radioactive decays follow first-order kinetics.)

Consider this mechanism for the enzyme-catalyzed reaction $$ \mathrm{E}+\mathrm{S} \stackrel{k_{1}}{\rightleftharpoons_{-1}} \mathrm{ES} \quad \text { (fast equilbrium) } $$ $$ \mathrm{ES} \stackrel{k_{2}}{\longrightarrow} \mathrm{E}+\mathrm{P} \quad(\text { slow }) $$ Derive an expression for the rate law of the reaction in terms of the concentrations of \(\mathrm{E}\) and \(\mathrm{S}\). (Hint: To solve for [ES], make use of the fact that, at equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.)

A factory that specializes in the refinement of transition metals such as titanium was on fire. The firefighters were advised not to douse the fire with water. Why?
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