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Chapter 14: Problem 58

List four factors that influence the rate of a reaction.

Short Answer

Expert verified
The rate of a reaction is influenced by four main factors: the concentration of reactants, temperature, the presence of catalysts, and the surface area of the reactants.

Step by step solution

01

Concentration of Reactants

The concentration of reactants is one of the factors that influence the rate of a reaction. As the concentration of reactants increases, the rate of reaction also usually increases, because the likelihood of particle collisions increases.
02

Temperature

The temperature is another important factor. The rate of reactions generally increases as the temperature increases because the particles move more quickly and interact with each other more at higher temperatures.
03

Catalysts

The presence of catalysts can also influence the rate of a reaction. Catalysts work by reducing the energy needed for a reaction to occur, which could increase the reaction rate.
04

Surface Area

Finally, the surface area of the reactants can influence the reaction rate. The larger the surface area, the greater the chance for particle collisions, which means the rate of the reaction could increase.

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Most popular questions from this chapter

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.)

(a) What can you deduce about the activation energy of a reaction if its rate constant changes significantly with a small change in temperature? (b) If a bimolecular reaction occurs every time an A and a B molecule collide, what can you say about the orientation factor and activation energy of the reaction?

The reaction of \(\mathrm{G}_{2}\) with \(\mathrm{E}_{2}\) to form \(2 \mathrm{EG}\) is exothermic, and the reaction of \(\mathrm{G}_{2}\) with \(\mathrm{X}_{2}\) to form \(2 \mathrm{XG}\) is endothermic. The activation energy of the exothermic reaction is greater than that of the endothermic reaction. Sketch the potential energy profile diagrams for these two reactions on the same graph.

Determine the overall orders of the reactions to which these rate laws apply: (a) rate \(=k\left[\mathrm{NO}_{2}\right]^{2} ;\) (b) rate \(=k\) (c) rate \(=k\left[\mathrm{H}_{2}\right]\left[\mathrm{Br}_{2}\right]^{\frac{1}{2}} ;\) (d) rate \(=k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]\)

For a first-order reaction, how long will it take for the concentration of reactant to fall to one-eighth its original value? Express your answer in terms of the half-life \(\left(t_{\frac{1}{2}}\right)\) and in terms of the rate constant \(k\)
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