The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
The rate of a reaction, average and instantaneous rate of reaction,order and molecularity of reaction, determination of Oder and molecularity, the integrated rate law of reaction, deferential rate law of reaction, zero order, first order and second order reaction, numerical for practice
Soluion and colligative propertries 2017nysa tutorial
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
class 12 chemistry.
for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
for more detail go my site
www.akchem.blogspot.com
This presentation consists of three topics that are:
1. conductance of electrolytic solution
2. Specific Conductance, Molar Conductance & Equivalent Conductance
3. Kohlrausch's Law
The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
The rate of a reaction, average and instantaneous rate of reaction,order and molecularity of reaction, determination of Oder and molecularity, the integrated rate law of reaction, deferential rate law of reaction, zero order, first order and second order reaction, numerical for practice
Soluion and colligative propertries 2017nysa tutorial
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
class 12 chemistry.
for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
for more detail go my site
www.akchem.blogspot.com
This presentation consists of three topics that are:
1. conductance of electrolytic solution
2. Specific Conductance, Molar Conductance & Equivalent Conductance
3. Kohlrausch's Law
This is a revision of my second order reaction rate presentation. It takes into consideration the fact that the product is formed at half the rate of disappearance of the reactant.
Chemical kinetics: the study of how fast chemical reactions occur.Specifically:
Rates of consumption of reactants and formation of products.
Response of chemical rates to changes in rxn conditions.
Identification of steps through which rxn takes place.
Reasons for study
Prediction of how quickly a rxn approaches equilibrium.
Understanding or elucidation of rxn mechanisms.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
3. Provides information about the time it takes for a chemical reaction to occur
4. Provides information about the series of elementary steps which lead to the formation of product
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
Provides information about the time it takes for a chemical reaction to occur
3. Provides information about the series of elementary steps which lead to the formation of product
My notes for A2 Chemistry Unit 4, typed by me and compiled from various sources. I cannot trace back where everything came from but again shall any intellectual property rights be violated, please comment /contact me and I will try my best to rectify them as soon as possible.
This is a review of electron repulsion to prepare students for any investigation that will help them understand how valence shell electron repulsion theory can predict the electron distribution around a central atom, and thus the shape of covalently bonded compounds. Designed for high school, it is probably useful on all levels including college 1.
A short introduction to the discovery, identity and health effects of the three typical radiations found in nature. Suitable for general or pre-AP chemistry.
Short introduction to what radioactive decay is and how to balance nuclear decay equations. Suggested you use after the introduction to alpha, beta and gamma radiation.
Lyrics to a song that may be used as a humorous "tail" to a thermodynamics lesson or lab. You may sing it to Gershwin's "Summertime" from Porgy & Bess.
This is a brief presentation outlining the three ways to draw electron configurations--using the periodic table, using the visual mnemonic, and using the ear memory.
MATATAG CURRICULUM: ASSESSING THE READINESS OF ELEM. PUBLIC SCHOOL TEACHERS I...NelTorrente
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Biological screening of herbal drugs: Introduction and Need for
Phyto-Pharmacological Screening, New Strategies for evaluating
Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
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Antifertility, Toxicity studies as per OECD guidelines
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
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students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Executive Directors Chat Leveraging AI for Diversity, Equity, and InclusionTechSoup
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
A Strategic Approach: GenAI in EducationPeter Windle
Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
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A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
1. Solving Kinetics Problems
Writing Rate Expressions from Balanced
Equations
Finding Reaction Order from [A]-time Data
Finding Reaction Order from Initial Rate
Finding k from [A] & Rate Data
Calculating ½ Life from k
Drawing Reaction Profile from Data
Creating Reaction Mechanisms from Rate
Law & Finding the Slow Step
2. Writing Rate Expressions from
Balanced Equations
The rate expression is not the rate law
It tells us what we are looking for in a rate
law experiment
Example: H2 (g) + I2 (g) → 2 HI (g)
Rate expression could be rate of
disappearance of hydrogen It tells you in
−
Rate = ΔH2 = 1 ΔHI
Δt
2 Δt
the lab what
to measure
3. Your turn
The equation is
−
−
Cu (s) + 2 Ag+ (aq) → Cu2+ (aq) + 2 Ag(s)
Write at least two expressions by which
we could measure the rate
Answers:
−
Rate = ΔCu = 1 ΔAg+ = ΔCu2+ = 1ΔAg
Δt
2 Δt
Δt
2 Δt
4. Finding Reaction Order from
[A]-time Data
Needed: a chart of concentration of a reactant we
want to study vs. time
Product: a fast graph of Ln[A] vs time or 1/[A] vs
time
If the Ln[A] v time graph is linear, it's first order
If the Ln[A] v time graph is a curve, it's 2 nd order
If [A] v time goes down in a linear fashion, it's
zero order (rare)
5. Your turn
Reactant A changes concentration with
time. Here is the data:
What is the order of the reaction in A?
Hint: find the natural log of each [A] and
graph on your graphing calculator
7. Your Turn
Butadiene changes concentration with time.
Here is the data:
Time (s)
0
[Butadiene] 0.01000
Mol/L
1000
1800
2800
3600
4400
0.00625
0.00476
0.00370
0,00313
0.00270
What is the order of the reaction in butadiene?
Again, find the natural log of each [A] and graph
on your graphing calculator.
8. Solution
Plotting LN[butadiene] vs time we get
This is not a straight line as shown by the straight line between
the first and last points, so the reaction must be 2nd order.
9. Finding Reaction Order from Initial
Rate
This is a favorite of test writers!
You are given concentrations of all
reactants and the rate of reaction for each
set of conditions
You must identify the controls and variables
and determine how the rate is affected
You are looking for doubling of rate when
concentration doubles (1st), or quadrupling
of rate when concentration doubles (2 nd)
10. Your Turn
SO2 + O2 → SO3
Given the following data, determine the
order of reaction in SO2 and O2
Look for doubling of concentrations with
other concentration held constant!
11. Solution
Given the following data, determine the
order of reaction in SO2 and O2
In 2 and 1, oxygen concentration doubles while SO2 is
held constant
12. Solution
Given the following data, determine the
order of reaction in SO2 and O2
In 2 and 1, rate of formation of the trioxide goes from
0.60 to 1.20, also a doubling
13. Solution
Given the following data, determine the
order of reaction in SO2 and O2
That means the rate is directly proportional to the
concentration of the oxygen gas, so the reaction is
first order in O2
14. Solution
Given the following data, determine the
order of reaction in SO2 and O2
When we look at Experiments 1 and 3, we see the
oxygen concentration is held constant, and the SO 2
concentration is doubling.
15. Solution
Given the following data, determine the
order of reaction in SO2 and O2
But at the same time, the rate of trioxide formation
goes from 1.2 to 4.8, which is a quadrupling. That is 2 2
times the initial rate, so the rate is going up faster
than the concentration.
16. Solution
Given the following data, determine the
order of reaction in SO2 and O2
This means that Rate = k[SO2]2
The reaction is 2nd order in SO2
17. Predicting Concentrations, Rates
Now that we have reaction order, let's see
if we can fill in the table.
The reaction is 1st order in O2 and 2nd order in SO2
18. Solutions
To find the oxygen in Exp 4, we see that
the rate is 17% lower than in Exp 1
The reaction is 1st order in O2 and 2nd order in SO2
19. Solutions
And the [SO2] is 33% lower than in Exp 1
That is predictable since Rx is 2nd order
The reaction is 1st order in O2 and 2nd order in SO2
20. Solutions
The change in sulfur dioxide accounts for
all the rate change, so oxygen is 0.20 M
0.20 M
The reaction is 1st order in O2 and 2nd order in SO2
21. Solutions
Now predict the rate of forming trioxide in
experiment 5
0.20 M
The reaction is 1st order in O2 and 2nd order in SO2
23. Solutions
The oxygen is 50% higher than in Exp 2,
so rate should be 50% higher, or 9.0 x
10-3
0.20 M
The reaction is 1st order in O2 and 2nd order in SO2
24. Solutions
But SO2 is 17% higher than in Exp 2, so
rate from that is 33% higher yet, 1.2 x 10 2
0.20 M
1.2 x 10-2 M/s
The reaction is 1st order in O2 and 2nd order in SO2
25. Finding k from [A] & Rate Data
Let's go with a first order reaction we have
already looked at:
Rate = -0.240[A] -2.49, from the equation of line
And k = negative of slope, or 0.240 here
26. Finding k from [A] & Rate Data
But suppose we have the data, but no
equation, and know it's first order
Look at Exp 1 and 2 and assure yourself that
the reaction is first order in A
27. Finding k from [A] & Rate Data
Look at Exp 1 and 3 and see that the
reaction is 2nd order in B
28. Finding k from [A] & Rate Data
Look at Exp 3 & 4 and see that the reaction
is 2nd order in C
29. Finding k from [A] & Rate Data
Thus the rate law is
Rate = k[A][B]2[C]2
30. Finding k from [A] & Rate Data
So solve for k and plug in the numbers
from any of the fully known data lines
K = Rate
[A][B]2[C]2
Rate = k[A][B]2[C]2
31. Finding k from [A] & Rate Data
So solve for k and plug in the numbers
from any of the fully known data lines
K = 2.85 x 1012
This is harder than anything on a test
Rate = k[A][B]2[C]2
32. Your Turn
Find the value of the rate constant:
2 NO (g) + Cl2 (g) → 2NOCl (g)
Data:
[NO]o mol/L
[Cl2]o mol/L
Initial Rate
Mol/L-min
0.10
0.10
0.18
0.10
0.20
0.36
0.20
0.20
1.45
First you must find the order of the reaction in both
reactants, and write the rate law, then plug in to solve
for k.
33. Solution
Find the value of the rate constant:
The rate law is Rate = k [NO]2[Cl2]
So k = (Rate)/[NO]2[Cl2] = 0.18 x 10-3 L2mol-2min-1
[NO]o mol/L
[Cl2]o mol/L
Initial Rate
Mol/L-min
0.10
0.10
0.18
0.10
0.20
0.36
0.20
0.20
1.45
First you must find the order of the reaction in both
reactants, and write the rate law, then plug in to solve
for k.
34. Calculating ½ Life from k
We'll stick with first order reactions here
Remember that t ½ = 0.693
k
Suppose the rate constant for a 1 st order
reaction is 0.18 x 10-3s-1 What is the halflife? If the initial concentration is 2.0 M,
what will it be after the reaction runs for 770
seconds?
35. Solution
Suppose the rate constant for a 1st order reaction is 0.18 x 103 -1
s What is the half-life? If the initial concentration is 2.0 M,
what will it be after the reaction runs for 770 seconds?
T ½ = 0.693 = 0.693 = 385 s
K
0.0018 s-1
Now 770/385 = 2.0 so that's 2 half-lives
In the first half-life, the concentration goes to 1.0 M
In the second half-life, the concentration goes to 0.50 M
36. Your Turn
A certain first-order reaction is 45.0%
complete in 65 s. What are the rate
constant and half-life for this process?
This is #37 on page 605
37. Your Turn
A certain first-order reaction is 45.0% complete in 65 s. What
are the rate constant and half-life for this process?
If [A]o = 100.0, then after 65 s, [A] = 55.0. In 1 st order Rxn,
LN([A]/[A]o = -kt, LN(55.0/100.0 = -k(65 s)
You do the arithmetic, but
K = 9.2 x 10-3 s-1 and t ½ = 0.693/k = 75 s
This is #37 on page 605
38. Drawing Reaction Profile from
Data
This should be a little familiar to you if you
recall the diagrams of endothermic and
exothermic reaction
We just add the activation energy and
diagram it like a hill the reactants have to
get over by colliding at the right energy and
orientation.
39. Drawing Reaction Profile from
Data
Draw a reaction energy profile for an endothermic
reaction with ΔH = +34 kJ/mol and a forward
activation energy of 66 kJ/mol. Calculate the
activation energy in the reverse direction.
40. Drawing Reaction Profile from
Data
Draw a reaction energy profile for an endothermic
reaction with ΔH = +34 kJ/mol and a forward
activation energy of 66 kJ/mol. Calculate the
activation energy in the reverse direction.
41. Your turn
Draw the reaction energy profile of an exothermic
reaction with a forward activation energy of 116
kJ/mol and a ΔH of -225 kJ/mol. Calculate the
activation energy in the reverse direction.
42. Your turn
Draw the reaction energy profile of an exothermic
reaction with a forward activation energy of 116
kJ/mol and a ΔH of -225 kJ/mol. Calculate the
activation energy in the reverse direction.
Ea for
reverse
direction is
341 kJ/mol
From UC Davis
43. Creating Reaction Mechanisms from Rate
Law & Finding the Slow Step
The rate law gives us a mathematical
picture of the initial and time-related
concentrations or pressures at a given
temperature.
However, to control reactions we need to
understand how they run. So we derive
reaction mechanisms from the rate law,
whenever possible.
44. Example
For the reaction H2 (g) + 2 ICl → I2 + 2 HCl the rate law
is found to be Rate = k [H2][ICl]
What is the most rational two-step mechanism that fits all
the information given?
First, a termolecular collision is almost never seen. So a
two-step mechanism is very reasonable.
The rate law implies that both hydrogen and ICl are
involved in the slow step.
45. Example
For the reaction H2 (g) + 2 ICl → I2 + 2 HCl the rate law
is found to be Rate = k [H2][ICl]
The rate law implies that both hydrogen and ICl are
involved in the slow step.
So we can reasonably say
• H2 + ICl → HI + HCl
• HI + ICl → I2 + HCl
Overall:
(slow)
(fast)
H2 (g) + 2 ICl → I2 + 2 HCl