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Chapter 16: Problem 93

How does the collision model account for the fact that a reaction proceeds faster when the concentrations of the reactants are increased?

Short Answer

Expert verified
The collision model accounts for the increased reaction rate when the concentrations of reactants are increased by explaining that higher concentrations lead to a higher frequency of collisions between reactant molecules and a higher probability of successful collisions. This ultimately results in a faster reaction rate.

Step by step solution

01

Understand the collision model

The collision model is a theory that explains how chemical reactions occur and why they have certain reaction rates. It is based on the idea that molecules must collide with each other with a certain minimum energy (called the activation energy) and in the correct orientation for a reaction to occur.
02

Explain the role of concentration in the collision model

In the collision model, the concentration of reactants plays an important role in determining the rate of the reaction. As the concentration of reactants increases, there are more molecules in a given volume. This higher molecular density leads to a higher frequency of collisions between the reactant molecules.
03

Relate increased concentrations to increased collision frequency

When the concentrations of reactants are increased, there are more molecules available to collide with each other in a given space. As a result, the likelihood of collisions between reactant molecules also increases. This means that there is a higher probability of successful collisions, leading to the formation of product molecules.
04

Describe how increased collision frequency affects reaction rate

According to the collision model, a faster reaction rate is observed when the number of successful collisions per unit time is larger. Since increasing the concentration of reactants leads to more frequent collisions, the probability of successful collisions also increases, resulting in a faster reaction rate. In conclusion, the collision model accounts for the fact that a reaction proceeds faster when the concentrations of the reactants are increased by explaining that higher concentrations lead to more frequent and successful collisions, ultimately increasing the reaction rate.

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Most popular questions from this chapter

For the reaction $$\mathrm{N}_{2}(g)+3 \mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{NCl}_{3}(g)$$ an analysis of an equilibrium mixture is performed. It is found that \(\left[\mathrm{NCl}_{3}(g)\right]=1.9 \times 10^{-1} \mathrm{M},\left[\mathrm{N}_{2}(g)\right]=\) \(1.4 \times 10^{-3} \mathrm{M},\) and \(\left[\mathrm{Cl}_{2}(g)\right]=4.3 \times 10^{-4} \mathrm{M} .\) Calculate \(K\) for the reaction.

At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. $$\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$$ Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations are found to be \(\left[\mathrm{N}_{2}\right]=0.041 \mathrm{M},\left[\mathrm{O}_{2}\right]=0.0078 \mathrm{M},\) and \([\mathrm{NO}]=4.7 \times 10^{-4} \mathrm{M} .\) Calculate the value of \(K\) for the reaction.

The reaction \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\) is exothermic as written. For the maximum production of ammonia, should this reaction be performed at a lower or a higher temperature? Explain.

Suppose the reaction system $$\mathrm{UO}_{2}(s)+4 \mathrm{HF}(g) \rightleftharpoons \mathrm{UF}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. Additional \(\mathrm{UO}_{2}(s)\) is added to the system. b. 5.0 mol of \(\mathrm{Xe}(g)\) is added to the system. c. The reaction is performed in a glass reaction vessel; HF(g) attacks and reacts with glass. d. Water vapor is removed. e. The size of the reaction vessel is increased.

At high temperatures, elemental bromine, \(\mathrm{Br}_{2}\), dissociates into individual bromine atoms. $$\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{Br}(g)$$ Suppose that in an experiment at \(2000^{\circ} \mathrm{C},\) it is found that \(\left[\mathrm{Br}_{2}\right]=0.97 \mathrm{M}\) and \([\mathrm{Br}]=0.034 \mathrm{M}\) at equilibrium. Calculate the value of \(K\).
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