15. Chemical Kinetics

Stoichiometric Rate Calculations

19.3: Reaction Rates and Stoichiometry

Chlorite is reduced by bromide in acidic solution according 
to the following balanced equation: 
ClO2 
-1aq2 + 4 Br-1aq2 + 4 H+1aq2S Cl-1aq2 + 
2 Br21aq2 + 2 H2O1l2
(a) If Δ3Br24>Δt = 4.8 * 10-6 M>s, what is the value of 
Δ3ClO2 
-4>Δt during the same time interval?

The rate is not independent of [NO2&#8211;].

The rate increases as [NO2&#8211;] increases.

Correct, the rate changes by the same factor as the concentration.

The rate increases by the same factor as [NO2&#8211;].

 Use the method of initial rates to determine the reaction order. 

Using the following data, determine the order of the reaction with respect to [NO2&#8211;]. <table><caption>Data Table for Three Experiments</caption><tbody><tr><th scope="col">Experiment</th><th scope="col">Initial [NH4+]</th><th scope="col">Initial [NO2]</th><th scope="col">Initial rate (M/s)</th></tr><tr><th scope="row">Experiment 1</th><td>0.24 M</td><td>0.10 M</td><td>7.2 &times; 10-6 M/s</td></tr><tr><th scope="row">Experiment 2</th><td>0.12 M</td><td>0.10 M</td><td>3.6 &times; 10-6 M/s</td></tr><tr><th scope="row">Experiment 3</th><td>0.12 M</td><td>0.15 M</td><td>5.4 &times; 10-6 M/s</td></tr></tbody></table>

The rate is not independent on the concentrations of the reactants.

The rate increases with increasing concentrations of reactants.

This is the order with respect to either of the reactants.

Correct, the reaction is first order with respect to each of the reactants.

The rate is affected by the same factor as the concentration change for either of the reactants.

 The overall order is simply the sum of the exponents. 

Using the data below (also from question 6), determine the overall order of the reaction. <table><caption>Data Table for Three Experiments</caption><tbody><tr><th scope="col">Experiment</th><th scope="col">Initial [NH4+]</th><th scope="col">Initial [NO2]</th><th scope="col">Initial rate (M/s)</th></tr><tr><th scope="row">Experiment 1</th><td>0.24 M</td><td>0.10 M</td><td>7.2 &times; 10-6 M/s</td></tr><tr><th scope="row">Experiment 2</th><td>0.12 M</td><td>0.10 M</td><td>3.6 &times; 10-6 M/s</td></tr><tr><th scope="row">Experiment 3</th><td>0.12 M</td><td>0.15 M</td><td>5.4 &times; 10-6 M/s</td></tr></tbody></table>

Stoichiometric Rate Calculations Concept 1

14.1 Rate Expressions and the Rate of Reaction | General Chemistry

Ammonia is manufactured in large amounts by the reaction 
N21g2 + 3 H21g2S 2 NH31g2 
(b) How is the rate of formation of NH3 related to the rate 
of consumption of N2?

The rate of the initial step involves the collision of two molecules of NO2.

When a mechanism has a slow initial step - the rate law usually only contains the reactants in the overall reaction.

rate = k[NO2]2

Correct, the rate only depends on the reactants in the first step of the mechanism.

 The slow step in the mechanism is the rate-limiting step.  The rate law is based on the slow step of the mechanism. 

Write the rate law for the following mechanism:Step 1: NO2 + NO2 &#8594; NO3 + NO&nbsp;&nbsp;&nbsp;&nbsp;(slow)Step 2: NO3 &#8594; NO + O2&nbsp;&nbsp;&nbsp;&nbsp;(fast)

Average Rate of Reaction

Introduction to reaction rates | Kinetics | AP Chemistry | Khan Academy

14.1 Rates and Rate Expressions

(a) Consider the combustion of hydrogen, 2 H21g2 +
O21g2 ¡ 2 H2O1g2. If hydrogen is burning at the rate
of 0.48 mol>s, what is the rate of consumption of oxygen?
What is the rate of formation of water vapor?

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[BOOK CHEM] Clutch Version

Intro to Chemical Kinetics

Chemical Kinetics is the study of factors affecting reaction rates, which examines the speed by which reactants are consumed to make products.

Average (General) Rate is the change in the concentration of a compound over a period of time.

Arrhenius Equation

The Arrhenius Equation&nbsp;illustrates the temperature dependence of the rate constant k.&nbsp;

Rate Law

Rate Law represents an equation for a chemical reaction that connects the reaction rate with the concentrations or pressures of the reactants and the rate constant.&nbsp;

Factors Influencing Rates

There are 4 major factors that directly influence how fast or slow a reaction proceeds.

When the rate of one compound is know, the rate of another compound is calculated through rate-to-rate comparison.

Collision Theory

According to Collision Theory:chemical reaction is successful when 2 energetic reactants successfully collide.

Integrated Rate Law

When we include the variable of time to our Rate Law then we obtain the Integrated Rate Laws.&nbsp;

Catalyst

Catalyst is a substance that increases the rate of reaction by lowering the Activation Energy (Ea) of a reaction.

Instantaneous Rate

<div title="Page 1">&nbsp;Instantaneous Rate is the rate a reaction at any particular point in time.</div>

Reaction Mechanism

<div title="Page 1">A Reaction Mechanism is a step-by-step sequence of elementary steps by which an overall chemical change occurs.</div>

Half-Life

Half-Life is the time it takes for half&nbsp;of a reactant to decay in a certain time period.

Energy Diagrams

Energy Diagram represents a curved plot illustrating the energies of reactants, products and transition states of a reaction.

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