How the Concentration Affects the Rate of the Reaction

Title Page Number Diagram of Apparatus display Risk discernment Table of Results Line of Best Fit chart Error parallel cadences Graph Gradients Graph Analysis Error Bars Analysis Evaluation Improvement Assessment Improved Experiment. dependability References Introduction For this data analysis project, I conducted and try aside to investigate how the absorption of an unpleasant affects the charge per unit of the response.I convey set up the experiments equipment as delivern on figure 1. As you eject converge by figure 1, I have procedured the chemical reaction between sodium thisoulphate solution and hydrochloric back breaker (HCL) to come up with gists that leave alone help me draw conclusions regarding the effects of the slow-wittedness of the acid. I decided to use this particular reaction due to the position that the product of the reaction between sodium thisoulphate and hydrochloric acid (HCL) is strikes of entropy which tend to turn the solution c loudy.As a result, the cross beneath the conical flask ( draw figure 1) would thaw/ become difficult to be seen when the reaction has thrown place. Therefore, the idea is that 50 cm? of sodium thisoulphate ar make to react with 5 cm? of hydrochloric acid that is of different tightness each conviction. The concentrations of hydrochloric acid apply varied from 0. 1 to 5 moles. aft(prenominal)wards, the cross is observed through the top of the conical flask until it because invisible. The cadence of which this happens is then recorded and monitored using a stopwatch.The attribute equation of this reaction is as follows The to a spicyer place symbol equation shows the reaction Sodium thisoulphate reacts with hydrochloric acid to form sodium chloride, water, strike of sulphur as headspring up as sulphur dioxide. The results that I recorded from this experiment were poor. This is because they were not entirely accurate and did not gather in sense. As a result, my teacher gav e me a different set of results that were recorded at different temperatures to examine and help me write up.The table of results (table 2), shows the results obtained at 3 different trials of the same experiment. The reason behind repeating the experiment 3 metres is to ensure that the results reliability is of a satisfactory level. After the experiment was conducted, I looked back at the equipment I used as well as the stairs I carried out during the process. I did so to recognize the risks associated with carrying out such experiments. To prevent or minify such risks in future experiments, I conducted a risk assessment that is shown on the following scalawag Risk Assessment Risk Damage Prevention Method Hydrochloric Acid (HCL) Hydrochloric acid is corrosive. Eye bulwark must be worn at all times during Therefore it can defile skin. the experiment. It can also damage eyes. Ensure it does not come into contact with skin and if it does rinse thoroughly. Conical flaskfu l (glass) Can roll down the bench Make sure apparatus made of glass ar not Broken glass can cut/damage skin. chipped. Wear gloves if possible Be thrifty when handling glass. Sodium Thisoulphate Inhalation may cause irritation and coughing. Avoid contact with eyes and skin. pelt and eye contact might cause irritation and Do not inhale on purpose. damage Paper 1. A risk of a base cut is possible. 1. C beful eon handling paper and if paper cut occurs rinse and do not come in contact with hydrochloric acid. Risk Assessment (Table 2) Analysis Outliers Table 2 summarises the results of this experiment. As you can see, a couple of outliers have occurred during the experiment. I decided that a difference of more than 30 seconds between a result and the others obtained from repeating the same experiment indicates that this result is an outlier. Therefore the two outliers are ringed on table 2, so that they are made clear. For instance, the results recorded for t he third experiment using 0. 1 moles concentrated hydrochloric acid is 583 seconds.This is clearly an outlier due to the fact that the other results are 683 and 626 seconds, reservation the result of 583 seconds clearly distant and therefore is classed as an anomaly. Another outlier that has occurred is the result for the 3rd trial using 4. 0 moles hydrochloric acid. Here the outlier is 132 seconds, while the other trials show results that vary from one hundred sixty to 165 seconds. Graph Analysis The first represent (figure 2) states the averages of the recordings. I have used a word of mouth of best fit on this graph to identify the trends between the results.Firstly, the graph shows overall that the experiment has bygone as expected. This is because it looks very similar to the graph in the chemistry text book as well as ones found on the internet. The general trend that is shown by this experiment (as seen on figure 2) is that as the concentration of the hydrochloric acid sum up, the rate of the reaction also increases, as the reaction takes less time to take place. Therefore, the experiment shows that the concentration of the acid is directly proportional to the rate of the reaction. From 0. to 0. 5 Moles As you can see by figure 2, when 0. 1 moles of hydrochloric acid were used, the reaction was at its slowest, taking 656 seconds to take place. From 0. 1 to 0. 5 moles, the rate of the reaction increased significantly with the reaction notwithstanding taking around half the time 379 seconds to take place. At the start, the line of best fit has a gradient of 0. 000152 moles per second (m/s). I worked this out using the equation x/y = 0. 1/656 = 0. 000152 m/s. At 0. 5 moles, the gradient of the graph increases rapidly to 0. 00132 m/s.This calculation reinforces that the reaction is at its slowest at the beginning with the sulphur precipitate taking the least amount of time to cloud the solution and causing the cross to become invisibile. This is beca use a low concentration of hydrochloric acid means that not as much molecules are available to bump around, making molecular strike much less likely (). From 0. 5 to 1 Moles From 0. 5 to 1 moles, the time taken for the reaction to take place decreases further as the rate of the reaction increases. Therefore the precipitate of sulphur is taking less time to form ().The gradient of the graph also increases as a result to 0. 00357 m/s. I have worked this out using the same equation as above x/y= 1/280. This indicates that the rate of the reaction commemorates on increasing as the concentration of the hydrochloric acid increases. From 1 to 2 Moles By increasing the concentration of the acid from 1 to 2 moles, the rate of the reaction kept on increasing by taking less time for the reaction to occur. This is again shown by the line of best fit on figure 2, which at this point in the graph has a gradient of 0. 0913 m/s (x/y = 2/219), which is nearly triple the gradient stated previously . The rate of the reaction is a measure of how quickly this reaction is taking place. As you can see by the negative correlation between the time and the molarity of the acid shown on figure 2, the rate of the reaction keeps on increasing as the concentration of the hydrochloric acid is increasing. This result is supported by the collision scheme. This theory indicates that for a reaction to occur, the particles or molecules must collide with each other to form a reaction.Infact, they shoot to collide hard enough for the reaction to become a successful one as well, since only a certain fraction of the total collisions actually result in a chemical substitute (). When those successful collisions occur, they have enough activation energy to break existing bonds and form new bonds, resulting in a chemical reaction and a new product being formed (). Increasing the concentration of a solution means increasing the amount of molecules that are available in that solution.Therefore, incre asing the concentration of the hydrochloric acid from 1 to 2 moles is increasing the amount of molecules in the acid that would be available to collide and cause a reaction. Therefore, this means that there would be more particles per dm?. The fact that more particles are available explains why the rate of the reaction becomes faster. This is because the more particles there are, the more successful molecular collision would be happening, which increases the rate of which the reaction occurs. This aspect of the collision theory is illustrated by the diagram belowThe clash Theory (figure 5) (). As you can see by the diagram above, the amount of collisions happening per second is a major factor that determines how quickly or slowly the rate of the reaction goes. Therefore a high concentration increases the chances of collisions and consequently results in an increase in the rate of the reaction. From 2 to 4 Moles When increasing the concentration of the hydrochloric acid again from 2 to 4 moles, the trend still obeys the collision theory as far as the increase in the rate of the reaction is concerned.This is reinforced by the dramatic gradient increase to 0. 025 m/s (x/y = 4/163), which is shown by figure 2 as well as 4. According to the collision theory, it is expected that when the concentration of the hydrochloric acid two-base hits, the rate of the reaction will tend to double as a result too. On the other hand this does not seem to be the fiber in this experiment, since the time take for the reaction to take place when 2 moles hydrochloric acid was used is 219 seconds, while it is 163 seconds when 4 moles hydrochloric acid is used.This indicates that the reaction happening at this experiment was not a perfect one. This could be as a result of human faulting or other factors affecting the rate of the reaction, which will be discussed later. From 4 to 5 Moles Finally, by increasing the concentration of the hydrochloric acid used from 4 to 5 moles, the rate of the reaction was increased to become at its highest during this experiment, with the steepest gradient of 0. 035 m/s (x/y = 5/141).This implies that the amount of successful molecular collisions here are the highest with the sulphur precipitate clouding the solution in the quickest rate of time (141 seconds). Thus, the cross disappeared at the quickest rate as well. Error Bars Analysis The second graph (figure 3) is a graph of error bars. Error bars show the retch of results. I have drawn this graph since it is a visual account of the experiments reliability and so, it would help me decide whether the experiment was accurate enough or not. As you can see, the size of the error ars on figure 3 varies from small to large ones. I have decided that a bar range of 5 small squares on the graph is a reasonable maximum to detect the experiments accuracy. So, every range bars that vary above 5 small squares show inaccurate set of results. The error bars drawn on figure 3 show that the results obtained from 0. 1 to 0. 5 moles are quite inaccurate. This is because the error bars illustrated for those set of results are relatively big, showing a difference of from 6 to 10 small squares. This implies that those results with big error bars are quite poor and lack accuracy.However, the rest of the experiments show relatively small error bars. In addition, the error bars seem to be getting small and smaller with a bar range that varies below 5 or 4 small squares. This proves that the results keep getting more and more accurate towards the end of the experiment which makes. Overall I believe that the results of this experiment are 71% accurate. This is because 5 out of 7 of the error bars had a small range, deviation 2 out of 7 of the error bars with rather big range bars. Evaluation