/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 9 The rate constant \((k)\) depend... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 9

The rate constant \((k)\) depends on which of the following (there may be more than one answer)? a. the concentration of the reactants b. the nature of the reactants c. the temperature d. the order of the reaction Explain.

Short Answer

Expert verified
The rate constant (k) depends on the nature of the reactants (b) and the temperature (c). The nature of the reactants affects the rate constant because different reactions have different rate constants depending on the reactants involved and the mechanism of the reaction. The temperature affects the rate constant, as the reactant molecules have more kinetic energy at higher temperatures, making it more likely that they will collide with sufficient energy to overcome the activation energy barrier. This is described by the Arrhenius equation: \(k(T) = Ae^{(-Ea/RT)}\).

Step by step solution

01

Factor a: Concentration of the Reactants

The rate constant (k) is a proportionality constant that relates the rate of a reaction to the concentrations of the reactants. However, the rate constant itself doesn't change with the concentration of the reactants. So, (a) is not a factor affecting the rate constant.
02

Factor b: Nature of the Reactants

The nature of the reactants affects the rate constant. Different reactions have different rate constants depending on the reactants involved and the mechanism of the reaction. For example, reactions involving ionic species usually have larger rate constants compared to those involving covalent species. So, (b) is a factor affecting the rate constant.
03

Factor c: Temperature

The temperature affects the rate constant. As the temperature increases, the rate constant increases as well, because the reactant molecules have more kinetic energy, making it more likely that they will collide with sufficient energy to overcome the activation energy barrier. This is described by the Arrhenius equation: \[k(T) = Ae^{(-Ea/RT)}\] where \(k(T)\) = rate constant at temperature T, A = pre-exponential factor, Ea = activation energy, R = gas constant, and T = temperature in Kelvin. So, (c) is a factor affecting the rate constant.
04

Factor d: Order of the Reaction

The order of the reaction affects the relationship between the rate of the reaction and the concentrations of the reactants, but it doesn't affect the rate constant itself. The rate constant is the proportionality constant in the rate law expression, and its value remains the same for a given reaction at a fixed temperature, regardless of the order of the reaction. So, (d) is not a factor affecting the rate constant. In conclusion, the rate constant (k) depends on the nature of the reactants (b) and the temperature (c).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following reactions would you expect to proceed at a faster rate at room temperature? Why? (Hint: Think about which reaction would have the lower activation energy.) $$2 \mathrm{Ce}^{4+}(a q)+\mathrm{Hg}_{2}^{2+}(a q) \longrightarrow 2 \mathrm{Ce}^{3+}(a q)+2 \mathrm{Hg}^{2+}(a q)$$ $$\mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)$$

The rate law for the decomposition of phosphine \(\left(\mathrm{PH}_{3}\right)\) is $$\text { Rate }=-\frac{\Delta\left[\mathrm{PH}_{3}\right]}{\Delta t}=k\left[\mathrm{PH}_{3}\right]$$ It takes \(120 .\) s for \(1.00 M\) PH \(_{3}\) to decrease to 0.250 M. How much time is required for \(2.00\space \mathrm{M} \mathrm{PH}_{3}\) to decrease to a concentration of \(0.350\space \mathrm{M} ?\)

The rate law for a reaction can be determined only from experiment and not from the balanced equation. Two experimental procedures were outlined in Chapter \(11 .\) What are these two procedures? Explain how each method is used to determine rate laws.

One reason suggested for the instability of long chains of silicon atoms is that the decomposition involves the transition state shown below: The activation energy for such a process is \(210 \space\mathrm{kJ} / \mathrm{mol}\), which is less than either the \(\mathrm{Si}-\mathrm{Si}\) or the \(\mathrm{Si}-\mathrm{H}\) bond energy. Why would a similar mechanism not be expected to play a very important role in the decomposition of long chains of carbon atoms as seen in organic compounds?

The activation energy for the reaction $$\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{CO}_{2}(g)$$ is \(125 \mathrm{kJ} / \mathrm{mol},\) and \(\Delta E\) for the reaction is \(-216 \mathrm{kJ} / \mathrm{mol}\). What is the activation energy for the reverse reaction \(\left[\mathrm{NO}(g)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{CO}(g)\right] ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.