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Effect of temperature on reaction rate
Effect of temperature on reaction rate
Effect of temperature on reaction rate
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Kinetic Factors
Shelby Sarna
Turki Alkhaldi
September 1, 2015
CHEM-2130-003
TA: Donald MᶜCormick
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
2 MnO_4^(1-) (aq)+5 C_2 O_4 H_2 (aq)+6 H^+ (aq)→2Mn^(2+) (aq)+10 CO_2 (aq)+8 H_2 O(l) Results: The experiments required the starting, ending, and total times of each run number. To keep the units for time similar, seconds were used. An example of how to convert minutes to
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1A and 2A were still dark purple and light purple (respectively) at the beginning of the experiment and 10 minutes after. 3A had a translucent top and a dark purple bottom. There was a clear distinction of color in run 3A, much like combining water with oil. Since the tubes were rinsed multiple times with distilled water, dirty test tubes were not the problem. The cause of this reaction, or there lack of, may have been the test tubes not being mixed very well for runs 2A and 3A. However, 1A should have no reaction because 0 drops of "C" _"2" "O" _"4" "H" _"2" were added. So, "C" _"2" "O" _"4" "H" _"2" could not reduce Mn"O" _"4" ^"1-" in the KMn"O" _"4" …show more content…
Exercise IV “Effect of Copper Metal” demonstrates how increasing the amount of copper increases the rate. Run 3D had the fastest speed of reaction at 74 seconds from start to finish when 4 inches of copper wire was added to the solution. Run 2D was next with 75 seconds containing a 2 inch copper wire, and then 1D was last with no copper wire and finishing at 137 seconds.
High temperatures act like a catalyst and speed up chemical reactions; therefore, in exercise V “Effect of Temperature,” run 1E had a faster speed of reaction than run 2E. This difference in speed was because the temperature of run 1E was 3 degrees (Celsius) higher than run 2E. Run 1E lasted 42 seconds while run 2E lasted 208 seconds. Heat acted like a catalyst in this experiment by speeding up the particles which allowed the particles to hit more
For both experiments, data were collected for thirty seconds.
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
Experimental: The experimental procedure outlined in the OU Physical Chemistry Laboratory Manual was followed without any deviations.
The higher the temperature of the solution, the faster the rate of reaction, and vice versa. This is because as the solution heats up the particles gain energy and begin to move faster and with more energy. This causes more successful collisions per minute and consequently a faster rate of reaction. We carried out an experiment in lesson, which involved placing marble pieces in hydrochloric acid.
This enzyme speeds up the break down of hydrogen peroxide into water and oxygen, as enzymes are biological catalysts. [IMAGE]The reaction: Hydrogen peroxide Water + Oxygen Catalase -------- [IMAGE] 2H2O2 2H2O + O2 Apparatus: Hydrogen Peroxide, Several sticks of celery, Stand, boss and clamp, 100ml conical flask, 25cm3 burette, 1800cm3 beaker, Rubber bung with delivery tube, Distilled water, Large container filled with water, 10cm3 measuring cylinder, 10cm3 syringe, 20cm3 syringe, Blender, Knife, Ceramic tile, Electronic balance (correct to 2 decimal places), Sieve, Stopwatch/timer. The variables: There are many possible variables in this investigation, such as pH, temperature, the concentration of substrate and the concentration of the enzyme.
We then put the stopwatch on and left them for half an hour. After we weighed each potato tube and recorded our results. We did the experiment twice. We did this to make sure our results were correct. Preliminary method: We did everything the same as in our other experiment except we
Every day before sleeping, I record the exact time and collect them to show the effectiveness of certain methods. This experiment could be divided into 3 steps:
The effect of these factors can be explained using collision theory. Reactions occur when the reactant particles collide, provided the colliding particles have enough energy for the reaction to take place. As the molecules approach their electron clouds repel. This requires energy – the minimum amount of which is called the ‘activation enthalpy’ - and comes from translational, vibrational, and rotational energy of each molecule. If there is enough energy available, this repulsion is overcome and the molecules get close enough for attractions between the molecules to cause a rearrangement of bonds and therefore an ‘effective’ reaction has taken place. The more collisions of particles with kinetic energy over the activation enthalpy that occur, the faster the overall reaction. During this investigation I am focusing on the effect of temperature and concentration while aiming to maintain other rate determining factors at a constant level in order to ensure reliable results.
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.
And the symbol equation for it is:. Na2S2O3 + 2HCl, S + SO2 + 2Na + H2O. Before conducting my experiment, I will research into, amongst other things, the factors that affect the rate of a reaction. This is so that I may have enough information to understand the effect of temperature on the rate of a reaction and also gain appropriate understanding to make a suitable prediction as to what the outcome of my experiment will be. Reactions occur when the particles of reactants collide together continuously.
The experiment used Potassium permanganate (KMnO4), a purple substance; Potassium dichromate (K2Cr2O7), a yellow substance; and Methylene Blue, a blue substance. These substances have molecular weights, 158 g/mole, 294 g/mole and 374 g/mole. A petri dish containing agar-water gel with three wells was obtained as shown in Figure 1. Each well was labelled as potassium permanganate, potassium dichromate and methylene blue. One drop of every prepared substance was carefully placed into its respective wells in the agar-water gel using a dropper. The petri dish was immediately covered to avoid the possible effects of other foreign factors. The substances, each having specific colors, spread in the agar-water gel as shown in
The time and rate changes from the first two the second run are striking. In the non-music group, participants ran even faster, with an average time of 5.81 seconds, or 14.21 miles per hour – which is about 1.4% - not a very impressive gain. The music group, however, ran their second dashes in an average of 5.80 seconds, or 14.38 miles per hour. Thus, although participants in the music-listening group had markedly slower control runs, they somehow ended up having a slightly faster second run than the non-music group. Their second runs were a whopping 5.7% faster than their controls, which equates to a change of almost 0.8 miles per
Looking at the table of results above and the graph, it is shown that the higher the temperature got, the shorter the reaction time. The obtained results have been plotted on a line graph of the temperature of hydrochloric acid (y-axis) against reaction time (x-axis). This line graph in fig.2 also clearly shows that as the temperature increases, so does the speed of the reaction, shown by a reduction in the time taken. This corroborates the collision theory, where as the temperature of particles increase, the particles gain more kinetic energy and react with each other upon collision. This is shown as to happen in the hydrochloric acid, where the hydrochloric acid particles collide more with the particles of the magnesium ribbon as the temperature was increased. The above graph shows a gradual sloping curve, which gets steeper at higher temperatures. This shows that the reaction will reach a peak rate of activity as the gaps between the temperature and reaction times continue to decrease. The experiment fulfills the aim and clearly shows that as the temperature of a reaction is increased so does it’s rate of reaction, proving the hypothesis to be correct.
In conclusion to the second experiment we saw that each beaker took from 7 to 18 minutes depending on the heat of the water. we saw that sample number 1 took 18 minuets with heat of 10 degree C. and sample number 2 took 15 with heat of 25 degree C. and sample number 3 took 7 minutes with heat of 70 degree C. Now that we noted that we can say that the diffusion of copper sulphate varies depending not the temperature with beaker number 3 started the diffuse in 7 min and the beaker number 1 took 18. so the hotter the water the faster the diffuse of the copper sulphate.
The first experiments investigate the order of reaction with respect to the reactants; hydrogen peroxide, potassium iodide and sulphuric acid by varying the concentrations and plotting them against 1/time. An initial rate technique is used in this experiment so ‘the rate of reaction is inversely proportional to time.’ To find the order of reaction in respect to the reactants, 1/time is plotted against the concentration of Hydrogen Peroxide using the equation: