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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 is a measure of how fast a chemical reaction occurs, expressed as the change in concentration of a reactant or product over a given period of time, in units of moles per liter per second (M/s). (b) Three factors that can affect the rate of a chemical reaction are: (1) Concentration: higher concentration of reactants leads to increased reaction rates. (2) Temperature: higher temperature increases the kinetic energy of particles, leading to higher reaction rates. (3) Catalysts: these substances can lower the activation energy and increase the reaction rate without being consumed themselves. (c) In a balanced chemical equation, the rate of disappearance of reactants is equal to the rate of appearance of products, as the stoichiometry of the balanced equation dictates the necessary ratio of reactants to products. However, this applies to the overall reaction and not necessarily to each individual reactant or product; rates may differ for individual species but will still obey the stoichiometry of the balanced equation.

Step by step solution

01

(a) Definition of Reaction Rate

A reaction rate is a measure of how fast a chemical reaction occurs. It is usually expressed as the change in concentration of a reactant or product over a given period of time, typically in units of moles per liter per second (M/s).
02

(b) Factors Affecting Reaction Rates

(1) Concentration: Increasing the concentration of reactants generally increases the rate of a chemical reaction, because there are more particles available to react, thus increasing the likelihood of collisions that lead to a reaction. (2) Temperature: Increasing the temperature generally increases the rate of a chemical reaction, as the increased kinetic energy of the particles allows them to collide with greater force and frequency. This leads to a higher chance of successful collisions (that is, collisions that result in a reaction). (3) Catalysts: Catalysts can affect the rate of a chemical reaction by lowering the activation energy, the minimum energy required for a reaction to occur. This allows for a greater number of successful collisions and increases the reaction rate. Note that a catalyst is not consumed in the reaction and can be recovered unchanged at the end of the process.
03

(c) Rate of Disappearance of Reactants vs. Rate of Appearance of Products

In a balanced chemical equation, the rate of disappearance of reactants is indeed equal to the rate of appearance of products. This is because the stoichiometry of the balanced equation dictates the necessary ratio of reactants to products in the reaction, so when one reactant is consumed, a certain amount of product is formed according to the balanced equation. However, it is important to note that this applies to the overall reaction and not necessarily to each individual reactant or product; rates may differ for individual species within the reaction but will still obey the stoichiometry of the balanced equation.

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Most popular questions from this chapter

(a) What is a catalyst? (b) What is the difference between a homogeneous and a heterogeneous catalyst? (c) Do catalysts affect the overall enthalpy change for a reaction, the activation energy, or both?

The enzyme carbonic anhydrase catalyzes the reaction \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HCO}_{3}{ }^{-}(a q)+\mathrm{H}^{+}(a q)\). In water, without the enzyme, the reaction proceeds with a rate constant of \(0.039 \mathrm{~s}^{-1}\) at \(25^{\circ} \mathrm{C}\). In the presence of the enzyme in water, the reaction proceeds with a rate constant of \(1.0 \times 10^{6} \mathrm{~s}^{-1}\) at \(25^{\circ} \mathrm{C}\). Assuming the collision factor is the same for both situations, calculate the difference in activation energies for the uncatalyzed versus enzyme-catalyzed reaction.

(a) Consider the combustion of ethylene, \(\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})+\) \(3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\). If the concentration of \(\mathrm{C}_{2} \mathrm{H}_{4}\) is decreasing at the rate of \(0.036 \mathrm{M} / \mathrm{s}\), what are the rates of change in the concentrations of \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) ? (b) The rate of decrease in \(\mathrm{N}_{2} \mathrm{H}_{4}\) partial pressure in a closed reaction vessel from the reaction \(\mathrm{N}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) is 74 torr per hour. What are the rates of change of \(\mathrm{NH}_{3}\) partial pressure and total pressure in the vessel?

Consider the following reaction: $$ 2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) $$ (a) The rate law for this reaction is first order in \(\mathrm{H}_{2}\) and second order in NO. Write the rate law. (b) If the rate constant for this reaction at \(1000 \mathrm{~K}\) is \(6.0 \times 10^{4} \mathrm{M}^{-2} \mathrm{~s}^{-1}\), what is the reaction rate when \([\mathrm{NO}]=0.035 \mathrm{M}\) and \(\left[\mathrm{H}_{2}\right]=0.015 \mathrm{M}\) ? (c) What is the reaction rate at \(1000 \mathrm{~K}\) when the concentration of \(\mathrm{NO}\) is increased to \(0.10 \mathrm{M}\), while the concentration of \(\mathrm{H}_{2}\) is \(0.010 \mathrm{M}\) ? (d) What is the reaction rate at \(1000 \mathrm{~K}\) if [NO] is decreased to \(0.010 \mathrm{M}\) and \(\left[\mathrm{H}_{2}\right]\) is increased to \(0.030 \mathrm{M}\) ?

For the elementary process \(\mathrm{N}_{2} \mathrm{O}_{5}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{NO}_{3}(g)\) the activation energy \(\left(E_{a}\right)\) and overall \(\Delta E\) are \(154 \mathrm{~kJ} / \mathrm{mol}\) and \(136 \mathrm{~kJ} / \mathrm{mol}\), respectively. (a) Sketch the energy profile for this reaction, and label \(E_{a}\) and \(\Delta E\). (b) What is the activation energy for the reverse reaction?
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