Kinetics Lab Report

Kinetics Lab Report
From the results, it is clear to say that the paper ramp had the most amount of kinetic energy as it did
not have as much friction acting on the marble; however, the plastic and sticky tape ramp had lower
amounts of kinetic energy as they had more friction acting on the marble. I found out that the marble
with the same mass and same velocity will have the same kinetic energy but having friction applied
to it would change the amount of time and distance it takes. In different common experiments that
others have done, they mentioned numerous possible cautions to check just in case to make sure that
the experiment runs smoothly. In different common experiments that other have done, they
mentioned numerous possible cautions to check just in case ... Show more content on
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Another element that could of affected the result was my motion of my hand caused on the marble
released into a tube at the release point as it could of had extra kinetic energy in rolling through the
tube and emerging to the launch point. However, I made sure that I would apply the same amount of
force when dropping the marble and to redo trials if my movement interfered with the results. I also
made sure that I released the marble at the right place instead of further up or down the tube
sometimes. In addition, another possible component that could influence my calculations was the
speed of my hand when stopping the timer. In order to made sure that my time was accurate, I had
placed the timer in front of the horizontal distance and utilized my camera to record the exact time.
This allowed me to be curtain about my precise time. I had learned from other experiments that
neglected air resistance has a effect on the experiments has it would affect the decrease of kinetic
... Get more on HelpWriting.net ...

Investigating the Kinetics of the Reaction Between Iodide...
PLANNING
Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions
By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in
potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will
do three sets of experiments changing first the concentration of iodide ions, then the concentration
of Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking
place. From these results, I hope to draw conclusions as to the effects of these changes to the
environment of the reaction on the rate and also determine the order of the reaction and the
activation enthalpy.
Background information ... Show more content on Helpwriting.net ...
In terms of log to the base 10 this is:
log k = log A –Ea/ 2.303 RT
Reaction between Iodine ions and peroxodisulphate ions
S2O82–(aq) + 2I–(aq)  2SO42–(aq) + I2(aq)
In order to make the reaction clearer, during my experiment I will add starch and a small known
amount of sodium thiosulphate (to act as a queching agent). The thiosulphate ions turn iodine back
to iodine ions:
2S2O32–(aq) + I2(aq)  S4O62–(aq) + 2I–(aq)
Which means that no starch–iodine colour will appear until all the thiosulphate has been used up.
The amount of time taken for this occur (and the reaction to suddenly turn blue) is the same amount
of time for the reaction to produce the equvilant amount of Iodine.
Apparatus
(For making up solutions) weighing boats scales Beaker (150cm3)
3 Volumetric flasks (250cm3)

Distilled water
Glass rod
(for concentraion and temperature change experiments)
4 thermometers (0–110ºC)
A large number of boiling tubes (roughly 50 depending on repeats)
5 Burettes with funnels for filling
5 Clamp stands (for burrettes)
Stopwatch
(for temperature change only)
Two large beakers (400cm3)
Chemicals
Freshly made starch solution
Pottasium Iodide (made to solution with conc. 1.00 mol dm–3)
Pottasium peroxodisulphate (made to solution with conc.

Kinetics of Hydrogen Peroxide
February 22, 2007
Chem. 1130
TA: Ms. Babcock
Room 1830 Chemistry Annex
PURPOSE OF THE EXPERIMENT
The major purpose of this experiment is to determine the rate law constant for the reaction of
hydrogen peroxide and potassium iodide. In this experiment, the goal will be to try to measure the
rate law constant at low acidity, since at low acidity, anything less than 1.0 x 10–3M, the effect of
the hydrogen ion is negligible. To calculate the rate, the experiment will have to utilize the rate
equation, which is expressed as Rate = k[H2O2]a[I–]b. At low acidity, the rate of the Hydrogen ion
will not change, from our equation:
H2O2 (aq) + 2I– (aq) + 2H+ (aq) → I2 (aq) + 2H2O ... Show more content on
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Once the timer starts, both group members are to watch for any reaction that occurs. The reaction
should yield a slight change in color. The appearing color will be light blue. Once a reaction is
noticeable, the timer is to stop the stopwatch and the group will record the time down in the
following data table. If the color you observe is a dark blue, then you have passed the reaction point
and you must start the experiment over.
The following data is the data that was collected in the lab. If you wish to see the calculations,
please refer to the calculation Page that follows this section.
[H2O2]: 0.1 M
Table: Collected Data for Rate of Reaction of H2O2
Solution Number 1 2 3 4 5
Time of Color Change 2280 sec 1260 sec 800 sec 390 sec 185 sec
Start Time 0.0 sec 0.0 sec 0.0 sec 0.0 sec 0.0 sec
∆t in seconds 2280 sec 1260 sec 800 sec 390 sec 185 sec
Rate = ∆[ H2O2] / ∆t 2.193E–07 M/s 3.968E–07 M/s 6.250E–07 M/s 1.282E–06 M/s

2.703E–06 M/s
Initial [H2O2] 0.005 M 0.005 M 0.005 M 0.01 M 0.02 M
Initial [I–] 0.0045 M 0.0090 M 0.0150 M 0.0150 M 0.0150 M
The calculations performed in this lab included calculating the amount of sodium thiosulfate in each
of the solutions, calculating the [H2O2] used up during the reaction in each solution, calculating the
initial [H2O2] in each of the five solutions, and calculating the initial [I–] in

Kinetic Study of a Solvolysis Lab Essay
Kinetic study of a Solvolysis (Sn1) Reaction
Aneadra Bowles
Adasia Rutledge
Krystal Flakes
Robert Grimes
Jasmine Ross
June 5, 2012
Purpose: The purpose of this experiment is to use kinetics to study a solvolyis reaction
Introduction: The purpose of this experiment is to understand the kinetics of the hydrolysis of t–
butyl chloride.The kinetic order of reaction was studied under the effects of variations in
temperature, solvent polarity, and structure. It is particularly observed in tertiarhalides i.e. in
SN1mechanism, Nucleophilic Substitution which is in 1storder. It is basically a reaction that
involves substitution by a solvent that pretendslikea nucleophile i.e. it donates electrons. The
reaction being in firstorder means ... Show more content on Helpwriting.net ...
After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with
the remaining NaOH until the colorless solution remained pink. The final volume was then
recorded. While solution #1 was heating the same process was repeated with solution#2 and the
second burette
Results
Kinetic Run#1 BuretteReading | Elapsed Timet=tn–to (sec) | Vt NaOH | (V–Vt ) | ln (V–Vo)(V–Vt) |
ln (V–Vo)(V–Vt) | v | T0 | | | | | 1 | T1 | 2:09 | 48 | 23.23 | 0.11 | 2 | T2 | 3:11 | 46 | 21.45 | 0.12 | 3 | T3 |
4:01 | 45 | 18.455 | 1.1 | 4 | T4 | 4:42 | 44 | 17.55 | 2.6 | 5 | T5 | 5:23 | 43 | 13.66 | 2.4 | | | | | | |
Kinetic Run#2 BuretteReading | Elapsed Timet=tn–to (sec) | Vt NaOH | (V–Vt ) | ln (V–Vo)(V–Vt) |
ln (V–Vo)(V–Vt) | 1 | 3:40 | 50 | 10.2 | 14.0 | | 2 | 5:40 | 48 | 5.0 | 12.54 | 0.1 | 3 | 7.73 | 46 | 4.3 | 12.67
| 0.44 | 4 | 8;34 | 44 | 3.45 | 10.44 | 1.33 | 5 | 10:17 | 42 | 3.5 | 7.656 | 2.0 | | | | | | |
Discussion
In this lab experiment we determined the kinetic rate constant for a solvoysis reaction and observed
how a change in polarity of the solvents affects the reaction rate. For the specific reaction that we
did in the lab we actually measured the formation of HCl since the rate of

Investigating the Kinetics of the reaction between Iodide...
PLANNING
Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions
By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in
potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will
do three sets of experiments changing first the concentration of iodide ions, then the concentration
of Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking
place. From these results, I hope to draw conclusions as to the effects of these changes to the
environment of the reaction on the rate and also determine the order of the reaction and the
activation enthalpy.
Background information
The ... Show more content on Helpwriting.net ...
Effect of Temperature
A basic law of physical chemistry is that an increase in temperature causes an increase in the rate of
any reaction. As the collision theory states, for a reaction to take place the particles need to collide.
If the temperature is increased, each particle has greater kinetic energy transferred from the heat
energy, and therefore is moving faster (the average speed of molecules is proportional to the square
root of the absolute temperature.) The faster the particles are moving, the more likely they are to
collide and therefore the faster the reaction. Also, the more energy transferred to each particle due to
increased temperature the more likely it is to surmount the activation enthalpy and again the higher
the number of effective collisions. As a general rule, the rate of a reaction doubles for every increase
of 10K in temperature.
The diagram below demonstrates the effect of temperature on the rate of a reaction. Despite the
initial increase in the energy of particles of a lower temperature, one can see that those at a higher
temperature eventually surpass and lead to an overall higher amount of particles with energy higher
than the activation enthalpy and therefore a greater number of effective collisions.
The exact relationship between temperature and rate of reaction was first proposed by a Swedish
chemist called Arrhenius in

The Importance Of Chemical Kinetics
Chemical kinetics studies and determines the rate or speed at which chemical or physical processes
occur (Oliver,n.d.)(Jircitano, n.d.). The rate of reaction is the speed at which the reactant in a
reaction transforms into products or the change in concentration of a chemical species over the time
taken for that change to occur (Oliver,n.d.)(Jircitano, n.d.)(Mack, n.d.)(Blackburn,n.d.). Chemical
reactions occur at many different rates and in aqueous or equilibrium systems this rate is dependent
on the variables such as the reactivity of reagents, initial concentrations, temperature induced
fluctuations and any means of catalysis. (Oliver,n.d.)(Jircitano, n.d.)(Blackburn,n.d.). In order to
measure rate the change in concentration in a particular reaction must be determined as well as the
time of which this occurred. However studying the concentration at any time during a reaction is
problematic since the reaction must be stopped and a sample must be removed both which
negatively affect accuracy. One class of reactions that enables the change in concentration to be
observed at a particular time is clock reactions. Ina clock reaction an initial induction phase precedes
a significant change in concentration of a particular species. (Preece, King, Billingham, 1999). The
rapid increase in concentration results in significant effects such as dramatic color change. There are
two types of clock reaction: 1. Induction where as small concentration grows till it results in

Chemical Kinetics: The Iodine Clock
Chemical Engineering Department
FIRST YEAR LABORATOY REPORT #1
Name: Shams Alizada
Experiment Title: Chemical Kinetics: The Iodine Clock Experiment Date : 13 October 2016
Submission Date: 20 October 2016 Supervisor: Rashid Akhundov
Contents
Synopsis 2
Introduction. 3
Safety Precautions. 3
Theory 3
Experimental Technique 4
Equipment and Apparatus. 5
Experimental Procedure. 5
Results 6
Discussion 7
Conclusion 8
References 8
Synopsis
The experiment concerning the iodine clock reaction was carried out to find ... Show more content
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Lime or soda must be poured on the contaminated floor and it must be cleaned until the floor gets
dry. While using pipette during an experiment, the starch solutions must be pipetted using the rubber
suction bulb, the solutions must not be pipetted by mouth. After checking the color and time, all the
solutions must be disposed in the aqueous residue bottle.
Theory
Iodine Clock is the reaction which includes the colorless compounds and after mixture, observance
the appearance of color in the solution: dark blue/purple. The color, depending on the temperature
and the concentration of the substances which react with one another, appears in a short time

interval. Rate of reaction for the experiment is calculated in the equation given below: reaction
rate=k×〖[A]〗^m×〖[B]〗^n
Here, m and n are called –reaction order, k is called– rate constant which depends on temperature.
There are the factors that can have impacts on the reaction rate of the compounds. As mentioned in
the collision theory (John Green & Sadru Damji), (Green, 2014) these factors involve the
concentration of substances. This experiment will also determine the concentration of H_2 O_2 on
iodide

Chemical Reaction Kinetics
Reaction Kinetics
Kinetics of reactions, otherwise known as chemical kinetics, is the study of how particles and bonds
between particles change in a chemical reaction over time. These changes can be viewed at a
molecular level through the use of reaction rates. Reactions rates tell us how fast or how slow the
change is happening at this level, or how the reaction depends on the time.
In Chapter 14 of the textbook, it was given that a chemical reaction only occurs if there is a collision
between particles. The greater the amount of particles, then the greater the amoutn of collisions in a
given amount of time, the faster the rate of the chemical reation. So the rate of a reaction depends on
the concentration of the particles in the reation. ... Show more content on Helpwriting.net ...
If a chemical reaction has a slow rate, a relatively small fraction of molecules reacts to form
products in a given period of time." (Chemistry, 557) This can be applied to the rate reactions for
chemicals. How much of the reactants are used in a certain amount of time to produce the products,
is called the rate of the reaction. When finding the reaction rate of a chemical reaction, many factors
need to be included. First, we need to know what we are looking for. In Chemistry Structures and
Properties, the author provides examples such as the speed of a car being expressed in miles per
hour, or weight lost in lbs per week. We would have speed and weight, respectively, as units for our
answers. In the reaction A2 + B2 –> 2AB, for every 1 mol of A2 and B2 used, 2 mols of AB are
produced. In a chemical reaction the reactants are used up in order to form the products. In this case
the A2 and B2 are the reactants and AB is the product.
In order to find the numerical rate of a reaction, more than just the balanced equation is needed. In
the gas example above, the rate at which the gas will be consumed, and the distance, or miles, is
needed in order to find how much will be needed. This is where rate laws come into effect. Rate
laws use the balanced equation to express the relationship between the reations rate and the
reactions concentration. (Chemistry,

Kinetics Of Acid Catalysed Propanone / Iodine Reaction
Alexander Unsworth – Tomlinson
Candidate Number: 9133
Kinetics of Acid–Catalysed Propanone/Iodine Reaction
Equation for the reaction :
CH3COCH3(aq) + I2(aq) ––> CH3COCH2I(aq) + H+(aq) + I–(aq)
Iodine + Propanone –> Iodopropanone + Hydrogen (cation) + Iodine (anion)
Introduction: Aims:
To vary the concentrations of each reactant along with the sulphuric acid in order to observe and
measure its effect on the overall rate of reaction in absorbance using colourimetry.
2) Calculate the a mean rate constant using orders of reactions and the rate equation allowing for the
overall order or reaction to be found.
3) Calculate the activation energy of the reaction using different versions of the Arrhenius equation.
4) Try and propose a mechanism for the reaction using the orders of reaction taking into account the
iodine, propanone and sulphuric acid.
Chemical Background:
Iodopropanone is formed from a redox reaction between iodine and propanone which is irreversible.
Hydrogen ions (H+) are used as a catalyst for the reactants and are disassociated from Sulphuric
acid. During the reaction the iodine solution turns from a dark brown colour into a colourless
solution this is because the iodine is reacting to produce the iodopropanone and the the colourless
iodine ions. The way I will be observing the progress of the reaction is by using a digital
colourimeter to measure the absorbance value of the change in colour.
Chemical Theory:

The Collision

Kinetic Energy Science Project
There is energy all around us. We have energy in our everyday lives but we normally don't think
about the energy being used. For example, a cup on a table, this is potential energy. It is not moving
and it is completely still on the table. When you're driving in your car you are using kinetic energy.
In this experience we are using potential, kinetic, and gravitational potential energy. We are using
these forms of energy, math, and science to test how fast an object will roll down a ramp.
Kinetic energy is energy due to motion in which case all moving objects have kinetic energy. For
example, a boulder rolling down a mountain has kinetic energy. All moving objects have kinetic
energy. In this experiment, we will use kinetic energy when we are rolling the object down the ramp.
This is kinetic energy because it is The object will be moving. Potential energy is stored ... Show
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You will need the books and the wood to make a ramp. You need a stopwatch to see how long it
takes for the object to roll down the ramp. You need paper and pencil to record how long it takes the
object to roll down the ramp. The first thing that you have to do to complete this experiment is to
create a ramp. Stack the number of books you have and place a The next thing that should be done is
to find the angles of the ramp. Next, you have to find an object to roll down the ramp 10 times. After
you roll the object down the ramp, record what you have found about the experiment. Doing this
experiment, I have found 10 different times it takes our object to roll down a ramp of two math
books and one science book. I have converted the seconds it takes for the object to roll down the
ramp to the number of feet per hour it takes for the object to roll down the ramp. After I converted
them to feet per hour, I created a frequency table and histogram to show my data I have

Kinetic Energy Lab Report
How does mass and velocity affect kinetic energy in an object?
If you do change the IV, the DV will also change. This supports my original hypothesis which stated
that mass and velocity do affect an object's kinetic energy.
This data was tested using a pound of soft, polymer clay, a small Jolly Rancher candy, ruler, pencil,
and a measuring tape. The Jolly Rancher weighed 6 grams. The pencil was placed underneath the
middle of the ruler for balance. On one end, I placed the Jolly Rancher and dropped the clay on the
other end. I started dropping the clay from 107 centimeters. The measuring tape was placed behind
the pencil and ruler. I then video–taped the event to pinpoint the exact launch height of the candy.
The first experiment had no force

Crystal Violet Kinetics Lab
Crystal Violet Kinetics In this Crystal Violet Kinetics Lab, many procedures were performed order
to experimentally determine the rate constant(k), for the rate of the reaction of the crystal violet
solution and sodium hydroxide. To start, a Beers Law calibration experiment was conduction. Also,
two kinetic experiments were ran using both 5ml and 10ml of sedum hydroxide in order to
determine the reaction order(k^1), of the sodium hydroxide. The Beers Law calibration experiment
used many concentrations of crystal violet solutions. Each of these solutions were test and analyzed
in order to determine the absorbance of each concentration The results were than graphed and
produced a slope of 1.00E05 with an intercept of –2.21E–02. After the

Analyzing The Potential Energy And Kinetic Energy Of A...
Learning Objective (s)
Knowledge: The students will analyze the gravitational potential energy and kinetic energy of a
pendulum.
They will be able to understand that a pendulum can have both kinetic energy and gravitational
potential energy as it moves from one extreme to the other. Student Friendly Learning Objectives
(Posted on the white board)
Knowledge: I can measure and analyze the gravitational potential energy and kinetic energy of a
pendulum.
I can understand that pendulums can have both kinetic energy and gravitational potential energy as
their bobs move from one extreme to the other.
Assessment
Assessment Strategy
Informal formative: I should notice that the sum of the KE and PE near the middle of the ramps is
nearly the same as the kinetic or potential energy at points 1 or 3 respectively.
The kinetic energy at point 2 should be smaller than that at point 3. Performance Expectation and
Evidence
All students are expected to meet the objectives.
The informal formative evaluations will indicate whether or not the students are making progress
towards the targets.
Using Assessment to Guide Instruction
Any responses deviating from the expected will indicate misconceptions, which will be addressed.
More time might be granted to fully understand the concept of energy conservation. **If they feel
like they need more practice, through practice problems, it will be granted (if Mrs. Driver deems it
appropriate).
Instructional Materials, Equipment, Technology, and

Calculate The Kinetic Energy And Energy Of An Object...
Calculating Energy
Introduction:
The objective of this lab was to calculate the kinetic energy and potential energy of an object
through experimenting with a car and measuring its velocity when passing through photogates while
carrying a certain amount of weights. In order to find kinetic and potential energy, we applied the
concepts of velocity and speed that we learned previously. This lab showed us the application of the
concepts we learned in class and how potential energy is converted into kinetic energy, and vice
versa.
Theory: write more!
The principle used in this lab was that energy is conserved. The total energy is distributed as either
kinetic energy or potential energy. Kinetic energy is caused due to motion and potential energy is
caused due to gravity. We used the following formulas to calculate kinetic and potential energy, and
percent difference:
P.E. = mgh, K.E. = 1/2(M+m)v^2, and % difference=|PE–KE|/KE*100%.
Experiment:
The materials used in this lab were an air track, a beam balance, a car, a meter stick, a meter stick,
pulley system, and weights. In the first portion of the lab, we measured the potential energy. My
group and I did this by measuring the height (100 cm) from the ground to the pulley and multiplied
that by the mass of the. After gathering the results for the potential energy which was surprisingly
easy to do, we moved on to the second portion of the lab, assembling data for the kinetic energy. We
started by weighing the car, which came out

Chemical Kinetics Lab Report
Review 3: Text Chemical kinetics is the study of rates and mechanisms of chemical reactions. In our
study of chemical kinetics, experimental data identifying the initial concentrations of reactants and
the instantaneous initial rates of multiple trials is used to determine the rate law for the reaction, the
order of the reactants, the overall reaction order, and the average rate constant. By comparing the
instantaneous initial rates and the initial concentrations of the reactants for two trials, it is possible to
deduce the order of each reactant. In order to determine the order of A, the two trials must be
selected such that the concentration of A changes while the concentration of B is held constant. In
this case, trial 1 and trial 3 or trial 2 and ... Show more content on Helpwriting.net ...
k=(0.103M–2s–1+0.103M–2s–1+0.103M–2s–1+0.103M–2s–1)/4=0.103 M–2s–1 The average rate
constant is 0.103M–2s–1. Combining everything, the rate law for the reaction is Rate=(0.103M–2s–
1)[A]2[B]1. We know that the reaction is 2A+2B→C+D. Based on the orders we calculated for A
and B, we know that this reaction is not an elementary reaction because both of the coefficients of A
and B are 2, which do not match the calculated orders of A and B, which are 2 and 1 respectively.
Also, if this were an elementary reaction, we would expect 3 molecules to perfectly collide with
each other, which is highly unlikely. As a result, it is more likely that there was an intermediate and
that multiple steps were involved. Through experimental data, we can not only determine the order
of reactants, but also the rate law, the average rate constant, and the overall order of the reaction.
Using the orders calculated, we can also determine the integrated rate plot that best represents the
reactants and the type of

Essay on Lab Report Kinetics of Chemical Reactions
Lab Report Kinetics of Chemical Reactions Kinetics of chemical reactions is how fast a reaction
occurs and determining how the presence of reactants affects reaction rates. In this experiment the
rate of reaction for Fe+3 and I– is determined. Because the rate of chemical reactions relates directly
to concentration of reactants, the rate law is used to find the rate constant, and calculated with
specified temperatures. Two catalyst reactants are used in the experiment, thiosulfate and starch, to
dictate the time of reactions. The order with respect to Fe+3 and I– is also determined by graphing
the slope of the log rate initial as a function of the log (Fe+3) or (I–). The activation energy is also
graphed with the rate constant ... Show more content on Helpwriting.net ...
.004 .0038 2.03 x 10–6 –2.4 –5.69 2. .008 .0078 4.47 x 10–6 –2.1 –5.35 3. .012 .0118 5.68 x 10–6 –
1.9 –5.25 Calculations: [Fe+3] initial: 1. .04 M Fe+3 x 10.00 mL/100.00 mL = .004 [Fe+3] initial 2.
.04 M Fe+3 x 20.00 mL/100.00 mL = .008 [Fe+3] initial 3. .04 M Fe+3 x 30.00 mL/100.00 mL =
.012 [Fe+3] initial [Fe+3] adjusted: 1. .004 [Fe+3] initial –2 x 10–4 = .0038 [Fe+3] adjusted 2. .008
[Fe+3] initial –2 x 10–4 = .0078 [Fe+3] adjusted 3. .012 [Fe+3] initial –2 x 10–4 = .0118 [Fe+3]
adjusted Rate initial = ½ [S2O3–2] initial / time (s) [S2O3–2] initial = .004 m x 10.00 mL / 100.00
mL = .0004 [S2O3–2] initial Rate initial for Combo #1, Combo #2, Combo #3: 1. ½ (.0004) / 98.34s
= 2.03 x 10–6 2. ½

Kinetic Energy Research Paper
Kinetic energy is the energy of mass in motion. The most important property of kinetic energy is its
ability to do work. Energy of motion is usually expressed as E=½ mv2 and as such, to change the
kinetic energy of an object, work must be done on it (Urry, 2017). Moreover, kinetic energy can be
elastic or inelastic, which is the transfer of energy from one body to another in a collision.
Additionally, kinetic energy can convert from one form of energy to another. Kinetic energy can be
stored and converted to potential energy because it has the potential to do work.Potential energy is
the energy that matter has because of its structure. It exists whenever an object has a position or
arrangement within a system.The potential energy of an object ... Show more content on
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The cellular work uses an exergonic process to start an endergonic one. Consequently, the change is
endergonic if energy enters the system and exergonic if free energy is released. In an endergonic
reaction, free energy increases, and in an exergonic reaction free energy decreases. An exergonic
reaction is unstable and has a negative change in free energy. Free energy (G) is the available energy
to do work on a system. If the system releases free energy, then it can do work. However, if the
energy is absorbed, then work can be done on it. A cell does three types of work: mechanical, active
transport, and chemical (Urry,2017). For example, mechanical work is the contraction of muscle
cells, active transport is the movement of molecules against a concentration gradient, and lastly, an
example of chemical work is the synthesis of polymers (Urry, 2017). The hydrolysis of ATP releases
energy that cells can use to do cell work and ATP turns into ADP + Pi. As such, ATP acts at the
immediate source of energy that powers cellular work, while also mediating energy coupling in

Chemical Kinetics Lab Report
Introduction
The principles of chemical kinetics is the study of reaction rates and the mechanism in a chemical
reaction.2 The rate of the chemical reaction can be represented as the change in concentration of a
solution with time. Also, the rate reaction can be express in an equation known as the rate law. The
rate law can be express as rate=f([A],[B],[C],...) (1) where the rate reaction is represented as a
function of the concentrations in the chemical equation with time.3 The general chemical reaction
can be shown as aA+bB→cC+dD (2)
Then using Eq. 2, to form the rate of consumption which is the reactant and the rate of formation is
the products
∂[D]/∂t=∂[C]/dt=–∂[A]/dt=–∂[B]/∂t (3) where the rate of reactant or product is instantaneous at a
given time.
The rate of the reaction can also be written using Eq. 1 as rate=k[A]^x [B]^y (4) where the
concentration are raised to a power are proportional and k is called the rate constant. The rate
constant is independent of the concentration but depend on the temperature.2 The exponents are
called the order of the reaction and the different type of order of reaction are determine by the sum
of the exponents.3 The first order rate law is shown as rate=k[A]^1=–∂[A]/∂t (5) using Eq. 3 an Eq.
4 and rearranging Eq. 5 to form
–∂[A]/[A] =k∂t (6)
Then integrating Eq. 6 at the initial time (t=0) for concentration of A to be [A]0 and [A]t at a later
time to form the limit of the integration for the first–order

Lab Report On Kinetics Of Alcohol Oxidation
Lab Instructor's Name: Zhen Qiao
Student's Name: Nhu Duong
Section # CHEM 102 – 110
Experiment #6
Date of the experiment: 01/29/2016
Title: KINETICS OF ALCOHOL OXIDATION
Drexel University Winter 2016
Introduction:
This report concerns the experiment of determining the order of reaction and the kinetic rate
constant of alcohol oxidation. This experiment relates to the knowledge of chemical kinetics, the
application of Beer's Law, and other calculations.
Chemical kinetics involves the examination of reaction rates, which are the speeds of chemical
reactions. There are chemical reactions which proceed in long periods of time as well as chemical
reactions proceeding in short periods of time. Regarding reaction rates, the reaction order and
kinetic rate constant are considered.
Take a general reaction in solution for instance: aA+bB⇌Product(s) The reaction rate is calculated
using the following function: rate=k〖[A]〗^x 〖[B]〗^y
Where [A] and [B] are the concentrations of A and B in the solution, unit: mol/L or M; x and y is the
reaction order of A and B respectively; k is the kinetic rate constant, its unit depends on the order of
the reaction.
The values of x and y are the partial order corresponding to A and B. The sum of x and y is the
overall reaction order. The values of x and y can be either negative or positive. They can also be
either integer or fractional. The reaction rate can be understood as how fast the reactants are
consumed or how fast the

Kinetic Reaction Lab
Introduction: On the word of Shelton (2018) in the General Chemistry Ⅱ Lab Manual, "Kinetics is
the study of the rates which chemical reactions occur at. The rate of reaction is dependent upon the
change of concentration over the change in time" (p. 14). The objection of this lab was to establish
the order of reaction with respect to persulfate ion and the overall rate constant. Experimental
Procedure: For this lab, you will need three beakers that have a volume of 150mL, 2 graduated
cylinders that have a volume of 10mL and a stopwatch (Shelton, 2018 p. 15). In between
experiments, you will want to clean the beakers and the graduated cylinders thoroughly to obtain
accurate results. Beaker 1 and 2 will need to be kept separate and each will have a graduated
cylinder of their own. ... Show more content on Helpwriting.net ...
As advised by Shelton, you should do it at least 2–3 times to ensure that acquire the most precise
data. The first time my partners and I conducting this experiment, we got a brown liquid that we
weren't quite confident was the color the liquid was supposed to be. Consequently, we completed the
experiment again and that time we were efficient to capture the results we expected. There are no
theories applicable to this lab. The objective of this experiment was to establish the order of reaction
with respect to persulfate ion and overall rate. A way I would compare my results with my
classmates is by inquiring them how they stirred their solution after they mixed the contents of
beaker 1 and 2 together. Did they use a stirrer, mix it by shaking the beaker in a circle or did they
mix the solution at all? A strength I experienced during this experiment is the consistency of the
contents in the second beaker. Although the amount of K_2 S_2 O_8 and K_s SO_4 varied
throughput the four experiments, they all yielded the same results. Which was a black color when
the contents of beaker 1 and 2 were mixed into beaker 3.

The Physics Of Mechanical And Kinetic Energies
The mechanical, gravitational potential and kinetic energies (measured and average) showed trends
with the masses of the balls. The big ball (larger mass) possessed more mechanical, gravitational
potential and kinetic energy than the small ball (see summary table above) whereas the ball with the
smaller mass possessed less energy correspondingly (3.9976 > 0.4588, 1.2242 > 0.0428, 6.1853 >
1.2242). This trend was consistent throughout all of the recorded results. This can be justified by the
equations of mechanical, gravitational potential and kinetic energy which all include mass meaning
a larger mass constitutes to more energy (see Background Information).
The calculated theoretical and measured values showed differences with the ... Show more content
This is the mechanical energy. When the balls lose height, it loses potential energy but gains speed
(thus gaining kinetic energy). At halfway down (0.5m), half of the potential energy has been
converted to kinetic energy but the mechanical energy remains constant (see Equation 3: Mechanical
Energy in Background Information and graph above). This is because of the Law of Conservation of
Energy; energy cannot be created or destroyed, only converted and transferred. Eventually, there is a
complete depletion of gravitational potential energy and only kinetic energy at 0m as all the
gravitational potential energy has been converted during free–fall. Once in contact with the floor, the
kinetic energy converted to elastic potential (deformation), sound and heat energy, then back to
kinetic energy when bouncing and gaining gravitational potential energy as the height increased.
The ball never goes back up to the height it was dropped; it only bounces to a new peak which is
lower than the original peak height. This is because the Law of Conservation of Energy does not
'give' the ball more kinetic energy to bounce back up after the energy has been converted and lost to
sound energy and heat energy whilst hitting the ground (hence the 'boing' sound it makes, which
proves the Law of Conservation of Energy). This alone proves the Law of Conservation of Energy,
as the ball never bounces back to the same peak. The ball should have a higher temperature than it
originally

Formal Report- Kinetics of Reaction: the Iodine Clock...
factors affecting the kinetics of reaction between peroxodisulfate (vi) and iodide
d. del prado1 and j. belano2
1 department of food science and nutrition, college of home economics
2 department of food science and nutrition, college of home economics university of the philppines,
diliman, quezon city 1101, philippines date submitted: january 7, 2013
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ABSTRACT
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In everyday life, several reactions are encountered, but still knowledge on how fast these occur and
the factors affecting it were still insufficient. This study ... Show more content on Helpwriting.net ...
On the first part, 2 beakers with different contents were prepared. 5 runs were prepared, and each
run had different volumes of the substances. The different runs for the effect of Peroxodisulfate (VI)
and iodide ion concentrations on reaction rate were presented on Appendix A. Each run had different
concentrations of substances to test the effect of the change in amount of concentration to the rate of
the reaction. Contents of beaker A and B were mixed; the timer was started immediately, and was
stopped once a blue color appeared in the mixture. [7] Once Peroxodisulfate (VI) ions and iodide
ions combine they produce I2 molecules which in turn reacted with the starch added to form a blue
color. I2 reacted with the starch as fast as it was produced. Hence, it was very difficult to measure
the rate of its reaction. So as to address the problem, S2O3 2– ion was added. This ion destroyed the
I2 by reducing it back to I– as fast as it was produced. The amount of S2O32– ion added was just
small so that it would not consume so much time. If the initial concentration of S2O32– ion was
kept very small, Δ[S2O32–] would be small and Δ[S2O82–] would be even smaller. Consequently,
there would be little change in the concentration of the reactants during the elapsed time Δt. This
was a necessary condition for the initial rates method. The rate of the reaction was

Kinetic Resolution
Intro Kinetic resolution of a various esters was conducted, where the esters differed by a single
substituent. The substituents para to the aromatic ring were a hydrogen, methyl group, fluorine,
bromine, and chlorine atoms. The varying para–substituents influence on efficiency of separating a
racemic mixture into an enantioenriched reactant and product was assessed. The esters were formed
from a given set of ketones as the starting material and reduced into a racemic alcohol followed by
acetylation; the product was a racemic mixture of esters(1). In contrast, the kinetic resolution itself
was conducted using the racemic ester produced from the acetylation, and introduced in the
presence of an enantioselective lipase in order to produce an ... Show more content on
Helpwriting.net ...
The hydrogen and methyl substituents had the greatest E–values, 12.4 and 10.8 respectively, when
compared to the halogen substituents whose E–values ranged from ~8–4 (9). This apparent trend
depicting halogens to having the lowest enantioselectivity goes against the hypothesis that was made
stating that halogens, specifically the ester with a bromine substituent would have the greatest
enantioselectivity. Though halogens may have a lower enantioselectivity value, this is mostly due to
their %ee rather than the actual percent conversion from ester to alcohol. Furthermore the esters
with halogenic substituents had the greatest percent conversion from ester to alcohol: bromine –
73.0%, fluorine – 43.0%, and chlorine 27.9% (9). This is compared to lower percent conversion
from the esters with a methyl or hydrogen substituent in the para position of the benzene ring;
values of 14.9% and 27.5% respectively (9). This would reflect that notion that since the halogenic
substituents are more electron withdrawing there was a greater inductive effect to stabilize the
tetrahedral intermediate, which lowers the activation energy resulting in a great percent conversion
of ester in to alcohol. However higher reactivity did not imply greater selectivity for the R–
enantiomer. In contrast to the high percent

Lab Repor Chemical Kinetics Essay
Abstract The "Chemical Kinetics" experiment was done to investigate the changes in the rate of
reaction under the effect of concentration, temperature, and presence of a catalyst. It was determined
that as the concentration of reactants and the temperature increases, the rate of the reaction increases
as well. Also, the reaction was run by the presence of catalyst, and the rate of the reaction increased
drastically in the presence of it. The order of the reaction with respect to each reactant was
calculated to be: x = 1 [I–], y = 1 [BrO3–], z = 2 [H+] by the method of initial rates. The average
rate constant was determined to be 26.7 M–3s–1, and the activation energy was calculated to be 49.6
kJ/mol. Introduction The whole purpose ... Show more content on Helpwriting.net ...
The reaction occurred under three different temperatures: 40ْ C, 10ْ C, and 0ْ C. The experiment in
this part was carried out just like part one. In flask 1, 10 mL of 0.010 M KI, 10 mL of 0.0010 M
Na2S2O3, and 10 mL of H2O were mixed. In flask 2, 10 mL of 0.040 M KBrO3 and 10 mL of 0.10
M HCl were mixed, and 3 drops of starch was added. Then, the two flasks were put in an ice bath
and cooled to about 10ْ C. Afterwards, the two solutions were mixed together while in the ice bath
with swirling until turning blue. The time was recorded. The reaction was done the same way for the
other two degrees (0ْ C, 10ْ C). If the water needed to be cold, ice was added, and if hot water was
needed, the water was heated. In the third part of the experiment, the reaction was carried out in the
presence of a catalyst. The influence of the catalyst on the rate of the reaction was investigated.
Again, mixture 1 from part one was used. In flask 1, 10 mL of 0.010 M KI, 10 mL of 0.0010 M
Na2S2O3 ,and 10 mL of H2O were mixed. In flask 2, 10 mL of 0.040 M KBrO3 and 10 mL of 0.10
M HCl were mixed, and 3 drops of starch were added. Also, one drop of 0.5 M (NH4)2MoO4,
ammonium molybdate, was added to Flask 2 which acted as a catalyst. The two solutions were
mixed until a blue color was formed and the stopwatch was stopped. All the

The Physics Of Chemical Kinetics
Investigations into the mechanics of chemical kinetics can reveal invaluable information relating to
the rates of reaction. There are numerable applications of reaction rates, knowledge in this area is
pivotal for industrial, commercial and research sectors. Thus, allowing them the ability to
manipulate a variety of factors of chemical reactions with the use of reaction rates. In the scope of
the kinetics of clock reactions, there is a range of information that can be obtained about reaction
rates (Shakhashiri, 1992).
A clock reaction is characterised by an abrupt colour change following an established time lag
(Lente et al, 2007). The induction period in a clock reaction is a result of low concentrations of the
clock chemical (i.e. the chemical that enables the final reaction). The induction period ends after the
total consumption of a limiting reagent, which initiates a short increase in the rate of product
formation, resulting in a visible colour change (Schmitz, 2010)(Lente et al, 2007). The reaction rate
of clock reactions is subject to factors including temperature, concentration, catalysis and inhibition.
These factors can be manipulated, thus changing the length of the induction period in a 'clock–like'
manner (Shakhashiri, 1992).
Changes in the rate of reaction can be described in terms of chemical equilibrium. "Chemical
equilibrium is a state in which the forward and reverse reactions take place at the same rate"
(Wilbraham et al, 2002). The relative

Physics: Why Kinetic Energy Needs To Swing
Physics is involved in almost everything that we do in life. Over the Thanksgiving break, I took my
niece to the park, as we were both swinging the swing set, I noticed that when swinging back and
forth, the swing resembled a pendulum oscillating back and forth. I had three thoughts while
swinging: what is the kinetic and potential energy it requires to swing; will my 3 year old niece
swing faster than me, since she weighs less; and lastly is it possible to swing above the support bar
of the swing.
According to Hyperphysics, the definition of kinetic of energy is: "energy of motion" ("Kinetic
Energy", 2013). The kinetic energy of an object is the energy it possesses because of its motion. The
formula that represents kinetic energy equation ... Show more content on Helpwriting.net ...
Which is the same as saying, the higher the elevation the greater the kinetic energy will be. As
mentioned before, kinetic energy of a swing can be described as the fast swinging motion going
back and forth.
Looking at these equations I was also able to answer my previous question, does the weight of a
person effect how fast someone will swing? The example above shows that speed does not depend
of mass. An adult will have the same speed of a small child, when they are released from the same
height. In the absence of friction, the velocity of an object falling under gravity does not depend on
the mass of the object.
Lastly, is it possible to swing over the support bar of the swing set? Although, some will argue that
they have in fact swung over the bar, ideally a regular person using their own power, on a regular
swing set will not be able to swing over a support bar. After doing a great deal of research on this
particular topic, I found a very thorough explanation, on Quroa, that explained why this would be an
impossible task. In order to make it over the bar, the centripetal acceleration at the top of the swing
would need to be greater than the acceleration due to gravity. Because you change kinetic energy to
potential energy as you go from the "front–end" to the "back–end" of the swinging motion, you lose

Chemical Kinetics: Enzymes Essay
Chemical Kinetics is the branch of chemistry that studies the speed at which a chemical reaction
occur and the factor that influence this speed. What is meant by the speed of a reaction is the rate at
which the concentrations of reactants and products change within a time period. Some reactions
occur almost instantaneously, while others take days or years. Chemical kinetics understanding I
used in the process of designing drugs, controlling pollution and the processing of food. Most of the
time chemical kinetics is used to speed or to increase the rate of a reaction rather than to maximize
the amount of product. The rate of a reaction is often expressed in terms of change in concentration
(Δ [ ]) per unit of time (Δ t). We can measure the ... Show more content on Helpwriting.net ...
An interesting result is obtained when the instantaneous rate of reaction is calculated at various
points along the curve in the graph of the change in concentration versus time. The rate of reaction
at every point on this curve is directly proportional to the concentration of the reactants at that
moment of time.
Rate = k(reactant concentration)
Because this equation is an experimental law that describes the rate of the reaction, it is called the
rate law for the reaction. The proportionality constant, k, is known as the rate constant. For general
reactions (aA + bB cC + dD) the rate law is (rate = k[A]x[B]y) where k is the rate constant and the
exponents x and y are numbers that must be establish experimentally. The values of the exponents in
the rate law indicate the order of the reaction with respect to each reactant. The sum of x and y is
called the overall reaction order.
Catalysts are one of the factors that extremely affect the rate of a reaction. Catalysts are substances
that speed up the rate of a reaction without being consumed themselves. When the reaction has
ended, you would have exactly the same mass of catalyst as you had at the beginning. One common
example are enzymes which are catalysts used to speed chemical reactions inside our body.
Enzymes bind for the time being to one or more of the reactants, substrate(s), of the reaction they

Kinetic And Potential Energy For Roller Coasters
Our roller coaster "The Explosion" shows the First Law of Thermodynamics, the first law states that
energy will be conserved. Our roller coaster conserves energy by reaching its highest peak and
flowing with the energy that it has built up. It shows many different types of energy. An example of
that would be Kinetic and Potential energy. Kinetic energy is the energy of movement and Potential
energy is energy stored in an object. Work and power however are not involved in the motion of our
rollercoaster. Work is done when force is done to a project an power is the rate at which work is
performed. Work is not being performed on "The Explosion" because is not always moving in the
same direction or speed. Therefore, by definition power can not

Kinetic Energy In A Roller Coaster Essay
Amusement parks are very cool, they also have a lot of science to them. You can easily find kinetic
energy in a roller coaster, since it has so much weight it can easily move fast when it touches a
maximum weight point. Also you will have potential energy in a rollercoaster as well, when the
roller coaster stops at the tip of the tracks it has potential energy and then turns into kinetic energy
when the brakes are taken off to release the roller coaster. You can feel the changes obviously when
the brakes are set off, you immediately feel the gravity and kinetic energy working when the gravity
pulls it down. Even though the roller coasters use potential energy they also use gravity, the gravity
pulls the whole rollercoaster down if it wasnt for the electrical force that the roller coaster ... Show
Kinetic Energy makes a one of the energy's that is being used in a rollercoaster. Kinetic energy is
what the rollercoasters use to go up a ramp. There are also other rides that use almost the same
concept. The freefall ride uses the concept, it's used by when the freefall ride is going up kinetic
energy is being performed. When a ride is in motion it will always be using a kind of energy even if
its just falling down with gravity. Most of the rides have potential energy. A rollercoaster has
potential energy when it stops. A rollercoaster usually stops at the top of the hill of when its about to
make a big loop. The roller coaster will have kinetic energy when it goes up the hill and it will have
kinetic energy when its detained at the top. Once it comes down it gains the kinetic energy back up.
the roller coaster also has the gravity to pull it down when it's falling. Depending on the weight of
the roller coaster is how much kinetic energy it will give out and the amount of weight that is also
extra to the

Kinetic Energy Lab Report
Speed, height, and mass do affect kinetic energy. In our lab work, we had to do multiple tests by
dropping a can onto a clay ball. We wrote down our data to prove that speed, height, and mass affect
kinetic energy. This is the lab data explained.
In our first lab, we had to drop different masses of cans from a height onto a 3cm clay ball and see
how much it got squished. Our data consisted of dropping a 418g, 227g, 624g, and 425g can from
30cm to a clay ball. For example, with a 418g can, the ball was squished down to 2.7cm while a
227g can squished a ball down to 2.9cm. This shows that the larger mass of the can, the more the
clay got squashed, so the more mass the object is, the more kinetic energy takes place.
In our second

Reaction Kinetics Essay
Reaction Kinetics: Rate of Reaction
Of Tertiary–Butyl Bromide
Purpose: The purpose of this experiment is to find the order of t–BB graphically, to find the k (rate
constant) at 0&#730; C and at room temperature, also to find the Ea (activation energy).
Principles: Several different chemical kinetic principles were used in this experiment. The reaction
rates of this chemical equation were determined experimentally. This then allowed the reaction
mechanisms (i.e. orders of each component, rate constant, etc.). These mechanisms were ultimately
determined to be compiled to form a rate law.
Rate = k[A]m[B]n
Integrated rate laws are used to determine concentrations of reactants at certain times. However, ...
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Data: Vo : 102mL Start time: 9:22:25 binf : 21.61mL
A Number Time to Colorless Total Sec bt (mL) (binf –bt) 1 9:25:05 160 2.00mL 19.61
2 9:28:04 339 4.00mL 17.61
3 9:35:34 789 6.00mL 15.61

Mass and Kinetic Energy Essay
Disk With Weight:
A 15 kg uniform disk of radius R = 0.25 m has a string wrapped around it, and a m = 3 kg weight is
hanging on the string. The system of the weight and disk is released from rest.
a) When the 3 kg weight is moving with a speed of 2.2 m/s, what is the kinetic energy of the entire
system? KETOT = KEwheel+KEweight = (1/2)(I)(w2)+(1/2)(m*v2) =(0.5* v2)(m+1/2M) =0.5*
(2.2^2)*(3+(.5*15)) J
b) If the system started from rest, how far has the weight fallen? H = KETOT/MG = 0.5*(2.2^2)*
(3+(.5*15))/(3*9.8) m
c) What is the angular acceleration at this point? Remember that a = αR, or α = a/R
Solve for acceleration by using ... Show more content on Helpwriting.net ...
Now, what is the translational kinetic energy of the sphere at the bottom of the incline? =mgh
(because there's no KErot, this is what ends up happening) 4.2*3.7sin(33)*9.8
Bar and Weights
A beam of mass mb = 10.0 kg, is suspended from the ceiling by a single rope. It has a mass of m2 =
40.0 kg attached at one end and an unknown mass m1 attached at the other. The beam has a length
of L = 3 m, it is in static equilibrium, and it is horizontal, as shown in the figure above. The tension
in the rope is T = 637 N.
a) Determine the unknown mass m1, at the left end of the beam. Sum of the forces = 0 because the
system is in equilibrium, so we can do F= ma, ma= 0, so F=0 m1g+m2g+m3g–Ft= 0
g(m1+m2+m3)=Ft m1= (Ft/g)–(m2+m3) 15
b) Determine the distance, x, from the left end of the beam to the point where the rope is attached.
Note: take the torque about the left end of the beam. =2.07
Hanging Sign
A sign has a mass of 1050 kg, a height h = 1 m, and a width W = 4 m. It is held by a light rod of

length 5 m that is perpendicular to a rough wall. A guy wire at 23° to the horizontal holds the sign to
the wall. Note that the distance from the left edge of the sign to the wall is 1 m.

Physics Of Kinetic Energy And Stopping Distance
Newton's law of inertia states that an object in motion will stay in motion until an equal and
opposite force stops it. In a collision, a driver's car is stopped by another object (Ex: another car, a
tree, a lamp post). Anything not attached to the car will continue to move forward because they are
not stopped by the force that halted the car. Therefore a person who is not wearing a seatbelt during
a collision would fly to the front of the car until they hit something (Ex: the dashboard, the wheel, a
car seat).The stopping distance of the vehicle going 60 mph would be four times greater than that of
the vehicle going 30 mph. This is because kinetic energy increases exponentially along with
velocity. From my prior knowledge in physics, I know that the formula for ... Show more content on
Helpwriting.net ...
Mass, kinetic energy, and stopping distance have a direct relationship so if the mass of the vehicle
goes up, the kinetic energy increases, and so does the braking distance. This can be proven by the
equation KE= 1/2mv2, as mention in the answer to the previous question. Assuming the vehicles'
velocities are the same, mass is directly correlated to kinetic energy. Kinetic energy and stopping
distance have a direct relationship, as explained in the previous answer.To prepare to enter sharp
curves, a driver should slow down. Lowering the velocity of a car decreases the kinetic energy in the
car. This means the braking distance would be shorter since there is less kinetic energy to convert.
Drivers that travel at a slower speed and have a short braking distance can pass through sharp curves
easier because they have more control over the vehicle and can stop if the vehicle gets too close to
the edge of the road.A reason why car crashes have different levels of injuries is that the force of
impact varies in distinctive situations. The force of impact in accidents depends on the size, weight,
and speed of the colliding

Potential Energy And Kinetic Energy In Soccer
Potential energy and kinetic energy: PE= mass x gravity x height KE= 1/2 MV2
The soccer ball has potential energy when it's in the air, when you kick the ball it turns into Kinetic
energy when it is moving. If the soccer ball is on the ground there is no potential energy because it's
related with height, when you kick the ball the kinetic energy from the player passes through the
ball.
Momentum: Momentum = mass velocity
Momentum is velocity of object times it's mass.
When we are striking the ball it transfers the momentum to the ball. While receiving the ball we use
our feet to stop the momentum of the ball by moving our feet back then attacking the ball slowly
enough that we can have more control of the ball.
Inertia: F = ma Is the resistance of the ball to acceleration, if there was no inertia when you kick the
ball it wouldn't go anywhere and immediately fall straight down to the ground and stop. ... Show
This includes wind flow, air speed and pressure. When a player strikes a ball the drag and force the
ball takes controls the trajectory, defiantly when the ball is spinning.
Velocity/speed:
Velocity is how fast you're moving, when you kick the ball it's putting Velocity on it. The more force
you put on the ball the more speed it has. Soccer players need to get the ball as fast they can, so they
need to increase the rate they change their position at.
Acceleration:
Acceleration= change in velocity * time interval Acceleration occurs when you kick the ball, the
change in acceleration while depend on the force of which you kick the ball. It also occurs when you
are running around the field. After the ball is kicked it actually starts to decelerate while in the air or
across the ground.
Newton's Laws of

Kinetics Lab
¬¬¬¬¬¬04/28/2010
Monday & Wednesday 7:40–10:30
Experiment #2 – Kinetics of the Decomposition of Hydrogen Peroxide
Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of
substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical
substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen
dioxide with the following reaction: 2 H202 (aq) 4 2 H20 (l) + 02 (g)
We can trap the oxygen gas created into a container thus showing the extent of the reaction and this
will show the rate in which oxygen is created and how the rate will change when we use different
initial concentrations. We do use a catalyst in this reaction to ... Show more content on
Helpwriting.net ...
It had a lot to do with the time and the amount of oxygen evolved. When holding the leveling bulb it
seemed that the longer I had to hold it level the harder it became to be as accurate. I would find my
arm getting tired and the bulb varying, which would also effect the times that we recorded. Another
thing that could have affected our results was not putting the stopper on the Erlenmeyer flask fast
enough, fumes from the formation of oxygen could have escaped before we got the stopper on,
causing error in the amount and time in which the oxygen was evolved.
Post Lab Questions:
1.
2.
3.

Difference Between Kinetic And Kinetic Energy
These things we use without even knowing we use them is things like our energy. Then when we use
these energies we continue to use every day. Then we use triangles everyday to even when we create
things to drive our car on and even to draw we use these things on a daily without even knowing.
For my background knowledge I know that you have all different types of energy and there is many
different types of colors. I also know that you can have triangles that can go along with angles and
height. When doing this you find many different ways to do things.Also knowing that they use
triangles for everything they can use all different types of triangles too.
Then you have all the energies like kinetic, potential, gravitational potential. ... Show more content
Our statistical question was made we had to think about how much the object could weight and how
hihet it would be so it would not break the board. With this experiment we are trying to find out how
much we can fit into the object or how much the object could weight. Also asking ourselves if we
had enough books to keep the boards stable and also asking our self if the object that is a can of
small winnes. Which adds up to our statistical question which is ( How long will it take to get the
object large/small amount of weight down the ramp.)
My hypothesis is that we can have the can of winners roll perfectly down our ramp.this because it is
a very small object and can build lots of speed. And it (the can of wines) they don 't have lots of
weight which can increase the possibilities. These are some energy 's / material that you have to
know to get also including that you need a ramp books and some sort of object.There are many
different types of energy one energy that is most know is kinetic energy and that is ( energy do to
movement). For example if there is a bowling ball hitting pins and knocking them over. The second
energy that is most known about is potential energy which is (Stored energy due to the interactions
of objects or particles). Also another energy to talk about is gravitational energy which is ( Stored
energy between a object when close to earth–hight –weight.).
For the procedures for

Kinetics
Section 1:
Kinetics is the study of the rate of chemical processes. The kinetics of the reaction between crystal
violet and NaOH was studied. In order to monitor crystal violet concentration as a function of time,
a spectroscopic colorimeter was used. What is the rate law for decolorization of crystal violet? In
order to figure this out, the rate of the reaction of crystal violet and sodium hydroxide must be
found. In this experiment, the initial goals were to determine the overall rate law for the rate of
decolorization of crystal violet in basic solutions as a function of time and to determine the rate law
for the reaction including the actual value of k; Rate = k[A]x[B]y. The rate of a reaction was
expected to depend on the concentrations ... Show more content on Helpwriting.net ...
Time) because it had a correlation closest to 1. All three orders were graphed and a linear regression
was used to see which graphed order was closest to 1. The order was determined by comparing the
concentration and time to the mathematical predictions made using the integrated rate laws.
Analyzing each graph and finding each correlation helped determine which graph was closest to 1.
The more concentrated a solution is, the higher the absorbance of that solution. This is due to Beer's
Law. The law measures the absorbance of a solution by determining how much light passes through
a solution. As the concentration of a solution increases, fewer wavelengths of light are able to pass
through the concentrated solution. The absorbance at 60 seconds was 0.573 (Figure 1: Table1). To
calculate the concentration (molarity), the Beer's Law equation was used, Abs = slope(m)+b.
Plugging in what is known into the Beer's Law equation resulted in 0.573 = 3.172e+004 + 0, where
the concentration is determined by M = 0.573–0/ 3.172e+004. So, the concentration at 60 seconds
using the equation (M = 0.573–0 / 3.172e+004) was 1.824e–5 M. The 1st order graph resulted in
k=0.006152 (Figure 1: Graph 1). Other groups also resulted in their decolorization of CV to be the
1st rate

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Kinetics Lab Report