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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 speed at which a chemical reaction occurs, typically measured in moles per liter per second (mol/L/s). It is the change in concentration of reactants or products over time. (b) Three factors affecting reaction rate are temperature, concentration of reactants, and the presence of catalysts. (c) Yes, the rate of disappearance of reactants is always the same as the rate of appearance of products, due to the Law of Conservation of Mass, which states that the total mass of reactants must equal the total mass of the products in a closed system.

Step by step solution

01

Define Reaction Rate

Reaction rate refers to the speed at which a chemical reaction occurs. It is the change in concentration of reactants or products over a specific period of time. The unit of reaction rate is typically moles per liter per second (mol/L/s).
02

Factors Affecting Reaction Rate

There are several factors that influence the rate of a chemical reaction. Three common factors include: 1. Temperature: Increasing the temperature typically increases the reaction rate because it provides more energy for the particles to collide and react. 2. Concentration of reactants: A higher concentration of reactants usually leads to a faster reaction rate as there are more particles available for successful collisions and reactions. 3. Catalysts: The presence of a catalyst can increase the reaction rate by reducing the energy barrier required for a reaction to occur, allowing the reactant particles to collide and react more easily.
03

Reactants Disappearance vs. Products Appearance Rate

Yes, the rate of disappearance of reactants is always the same as the rate of appearance of products in a chemical reaction. This is because, according to the Law of Conservation of Mass, the total mass of the reactants must equal the total mass of the products in a closed system. As a result, when reactants are consumed and disappear, products are formed and appear at the same rate.

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Most popular questions from this chapter

As shown in Figure 14.23 , the first step in the heterogeneous hydrogenation of ethylene is adsorption of the ethylene molecule on a metal surface. One proposed explanation for the "sticking" of ethylene to a metal surface is the interaction of the electrons in the \(\mathrm{C}-\mathrm{C} \pi\) bond with vacant orbitals on the metal surface. (a) If this notion is correct, would ethane be expected to adsorb to a metal surface, and, if so, how strongly would ethane bind compared to ethylene? (b) Based on its Lewis structure, would you expect ammonia to adsorb to a metal surface using a similar explanation as for ethylene?

(a) A certain first-order reaction has a rate constant of $2.75 \times 10^{-2} \mathrm{~s}^{-1}\( at \)20^{\circ} \mathrm{C}\(. What is the value of \)k$ at \(60^{\circ} \mathrm{C}\) if $E_{a}=75.5 \mathrm{~kJ} / \mathrm{mol} ?(\mathbf{b})\( Another first-order reaction also has a rate constant of \)2.75 \times 10^{-2} \mathrm{~s}^{-1}\( at \)20^{\circ} \mathrm{C}$. What is the value of \(k\) at \(60^{\circ} \mathrm{C}\) if $E_{a}=125 \mathrm{~kJ} / \mathrm{mol} ?(\mathbf{c})$ What assumptions do you need to make in order to calculate answers for parts (a) and (b)?

The reaction $2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)\( is second order in \)\mathrm{NO}$ and first order in \(\mathrm{O}_{2} .\) When \([\mathrm{NO}]=0.040 \mathrm{M}\) and \(\left[\mathrm{O}_{2}\right]=0.035 \mathrm{M},\) the observed rate of disappearance of \(\mathrm{NO}\) is $9.3 \times 10^{-5} \mathrm{M} / \mathrm{s} .(\mathbf{a})\( What is the rate of disappearance of \)\mathrm{O}_{2}$ at this moment? (b) What is the value of the rate constant? (c) What are the units of the rate constant? (d) What would happen to the rate if the concentration of NO were increased by a factor of \(1.8 ?\)

Which of the following linear plots do you expect for a reaction $\mathrm{A} \longrightarrow$ products if the kinetics are (a) zero order, (b) first order, or (c) second order?

Indicate whether each statement is true or false. (a) If you compare two reactions with similar collision factors, the one with the larger activation energy will be faster. (b) A reaction that has a small rate constant must have a small frequency factor. (c) Increasing the reaction temperature increases the fraction of successful collisions between reactants.
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