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Chapter 14: Problem 17

(a) What is meant by the term reaction rate? (b) Name three factors that can affect the rate of a chemical reaction. (c) Is the rate of disappearance of reactants always the same as the rate of appearance of products?

Short Answer

Expert verified
(a) Reaction rate refers to the change in the concentration of reactants or products per unit time, typically represented as moles per liter per second (M/s). (b) Three factors that can affect the rate of a chemical reaction include the concentration of reactants, temperature, and the presence of catalysts. (c) The rate of disappearance of reactants is directly related to the rate of appearance of products, but their rates may not always be the same. This depends on their stoichiometric coefficients in the balanced chemical reaction equation.

Step by step solution

01

(a) Defining "reaction rate"

Reaction rate refers to the speed at which a chemical reaction occurs, or more specifically, the change in the concentration of reactants or products per unit time. It is typically represented as moles per liter per second (M/s).
02

(b) Factors affecting reaction rate

There are several factors that can influence the rate of a chemical reaction: 1. Concentration of reactants: As the concentration of the reactants increases, the rate of reaction generally speeds up because there is an increased likelihood that the reacting particles will collide and interact with each other. 2. Temperature: An increase in temperature generally results in an increased reaction rate, as the particles have more kinetic energy and collide more frequently and with greater force. This increases the chances of successful collisions, which leads to faster reactions. 3. Catalysts: Catalysts are substances that can significantly speed up the rate of a chemical reaction without being consumed by the reaction itself. They work by lowering the activation energy needed for the reaction to occur (i.e., they provide an alternative reaction pathway with a lower energy barrier).
03

(c) Relationship between reactant disappearance and product appearance rates

In most chemical reactions, the rate of disappearance of reactants is directly related to the rate of appearance of products. According to the law of conservation of mass, matter cannot be created or destroyed, only converted from one form to another. Thus, when reactants are transformed into products, the total amount of mass in the reaction system should remain the same. However, if there are multiple reactants and products involved in a chemical reaction, we can't say that the rate of disappearance of one reactant is the same as the rate of appearance of one product. This is determined by their stoichiometric coefficients in the balanced chemical reaction equation. If the stoichiometric coefficients are the same for reactants and products, their rates of disappearance and appearance will be equivalent. Otherwise, we must compare the rates of disappearance and appearance according to their stoichiometric coefficients.

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Most popular questions from this chapter

(a) In which of the following reactions would you expect the orientation factor to be least important in leading to reaction: \(\mathrm{NO}+\mathrm{O} \longrightarrow \mathrm{NO}_{2}\) or \(\mathrm{H}+\mathrm{Cl} \longrightarrow \mathrm{HCl}\) ? (b) Does the orientation factor depend on temperature?

The addition of NO accelerates the decomposition of \(\mathrm{N}_{2} \mathrm{O},\) possibly by the following mechanism: $$\begin{array}{c}{\mathrm{NO}(g)+\mathrm{N}_{2} \mathrm{O}(g) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{NO}_{2}(g)} \\ {2 \mathrm{NO}_{2}(g) \longrightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)}\end{array}$$ (a) What is the chemical equation for the overall reaction? Show how the two steps can be added to give the overall equation. (b) Is NO serving as a catalyst or an intermediate in this reaction? (c) If experiments show that during the decomposition of \(N_{2} \mathrm{O}, \mathrm{NO}_{2}\) does not accumulate in measurable quantities, does this rule out the proposed mechanism?

What is the molecularity of each of the following elementary reactions? Write the rate law for each. \(\begin{array}{l}{\text { (a) } \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{Cl}(g)} \\ {\text { (b) } \mathrm{OCl}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HOCl}(a q)+\mathrm{OH}^{-}(a q)} \\\ {\text { (c) } \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NOCl}_{2}(g)}\end{array}\)

Consider the hypothetical reaction \(2 \mathrm{A}+\mathrm{B} \longrightarrow 2 \mathrm{C}+\mathrm{D}\) . The following two-step mechanism is proposed for the reaction: $$ \begin{array}{l}{\text { Step } 1 : \mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{X}} \\ {\text { Step } 2 : \mathrm{A}+\mathrm{X} \longrightarrow \mathrm{C}+\mathrm{D}}\end{array}$$ \(X\) is an unstable intermediate. (a) What is the predicted rate law expression if Step 1 is rate determining? (b) What is the predicted rate law expression if Step 2 is rate determining? (c) Your result for part (b) might be considered surprising for which of the following reasons: (i) The concentration of a product is in the rate law. (ii) There is a negative reaction order in the rate law. (ii) Both reasons (i) and (ii). (iv) Neither reasons (i) nor (ii).

Based on their activation energies and energy changes and assuming that all collision factors are the same, rank the following reactions from slowest to fastest.\( \begin{aligned} \text { (a) } E_{a} &=45 \mathrm{kJ} / \mathrm{mol} ; \Delta E=-25 \mathrm{kJ} / \mathrm{mol} \\ \text { (b) } E_{a} &=35 \mathrm{kJ} / \mathrm{mol} ; \Delta E=-10 \mathrm{kJ} / \mathrm{mol} \\ \text { (c) } E_{a} &=55 \mathrm{kJ} / \mathrm{mol} ; \Delta E=10 \mathrm{kJ} / \mathrm{mol} \end{aligned}\)
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