15. Chemical Kinetics

Instantaneous Rate

Drawing a tangent to find instantaneous rate of reaction

The rate of disappearance of HCl was measured for the
following reaction:
CH3OH1aq2 + HCl1aq2¡CH3Cl1aq2 + H2O1l2
The following data were collected:
Time (min) 3HCl 4 1M2
0.0 1.85
54.0 1.58
107.0 1.36
215.0 1.02
430.0 0.580
(d) Graph [HCl]
versus time and determine the instantaneous rates in
M>min and M>s at t = 75.0 min and t = 250 min.

Instantaneous Rate of Change

21.1.3 - Instantaneous Reaction Rates

From a plot of the concentration–time data in Worked 
Example 14.9, estimate: 
(b) the initial rate of decomposition of NO2.

Consider the decomposition of dinitrogen pentoxide:2 N2O5 (g) → 4 NO2 (g) + O2 (g)What is the instantaneous rate of this reaction at 20 seconds?<img src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/398922c6"class="fr-fic fr-dii">

(c) As a reaction proceeds, does the instantaneous reaction
rate increase or decrease?

Consider the reaction: 
H2( g) + Br2( g) ¡ 2 HBr( g) 
The graph shows the concentration of Br2 as a function of time. 
 
a. Use the graph to calculate each quantity: 
(iii) the instantaneous rate of formation of HBr at 50 s

Instantaneous Rate Example 1

Average versus Instantaneous Reaction Rates

From the plot of concentration–time data in Figure 14.1, 
estimate: 
(b) the initial rate of decomposition of N2O5.

Consider the reaction:
2 H2O2(aq) ¡ 2 H2O(l ) + O2( g)
The graph shows the concentration of H2O2 as a function of
time.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/8126c9a81fb69758-1665491981251.jpg" alt="" />
Use the graph to calculate each quantity:
c. the instantaneous rate of formation of O2 at 50 s

From a plot of the concentration–time data in Worked 
Example 14.9, estimate: 
(a) the instantaneous rate of decomposition of NO2 at 
t = 100 s.

Finding Instantaneous Rate | Rate of Reaction

The isomerization of methyl isonitrile 1CH3NC2 to acetonitrile
1CH3CN2 was studied in the gas phase at 215 C,
and the following data were obtained:
Time (s) 3CH3nC4 1M2
0 0.0165
2000 0.0110
5000 0.00591
8000 0.00314
12,000 0.00137
15,000 0.00074
(d) Graph 3CH3NC4
versus time and determine the instantaneous rates in M>s
at t = 5000 s and t = 8000 s.

Instantaneous Rate Concept 1

From the plot of concentration–time data in Figure 14.1,
estimate:
(a) the instantaneous rate of decomposition of N2O5 at
t = 200 s.

Consider the reaction:
H2( g) + Br2( g) ¡ 2 HBr( g)
The graph shows the concentration of Br2 as a function of time.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/0d40a3af5715c5f2-1660224256666.jpg" alt="" />
b. Make a rough sketch of a curve representing the concentration of HBr as a function of time. Assume that the initial
concentration of HBr is zero

Use the information in Table 14.1 and Figure 14.1 to estimate 
the instantaneous rate of appearance of NO2 at 
t = 350 s by calculating the average rate of appearance of 
NO2 over the following time intervals centered on t = 350 s. 
(a) 0 to 700 s (b) 100 to 600 s 
(c) 200 to 500 s (d) 300 to 400 s 
Which is the best estimate, and why?

Average Reaction Rate and Unique Average Reaction Rate

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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 Rate of Reaction

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.

Stoichiometric Rate Calculations

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.

<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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