The effect of concentration on rate of reaction was investigated Essay Example for Free

The effect of assimilation on stride of chemical reply was investigated EssayAnalysis1. How does reaction tell deepen according to preoccupancy?Based on our processed data, the lower the concentration the high-speed the reaction. This also means that the higher the concentration, the slower the reaction.2. Why is the like wool plug needed?The cotton wool plug is needed to absorb the amount of coulomb dioxide released. It acts as a sponge in absorbing the gas expelled from the conical flaskful. The cotton wool is weighed beforehand and then after absorbing one C dioxide, to find the mass of coke dioxide released. The amount of speed of light dioxide released can be used to calculate the roll of reaction.3. Why is thither no further loss in mass at the later conviction intervals?Eventually, there arent enough remaining moles of HCl to react with the calcium carbonate marble chips. Thus, there is no more than reaction and there is no carbon dioxide to be expelled.4. How could reaction rate be calculated from your graph?The first graph shows the loss of carbon dioxide over quantify. In this experiment, the rate of a reaction whitethorn be measured by following the rate at which carbon dioxide is formed. It is equivalent to the amount of carbon dioxide formed divided by time. The gradient of the graph can be used to calculate the rate of reaction, because the gradient is equal to a motley in the y values over a change in the x values. In this graph, it would be equivalent to a change in the loss of carbon dioxide over a change in time. This shows the rate of reaction and how fast it is going. Based on the graph, the bluff the slope, then the faster the reaction and vice versa.Conclusion and EvaluationIn this experiment, the effect of concentration on rate of reaction was investigated. We did this by reacting marble chips (calcium carbonate) with hydrochloric blistering, and recording the expelled mass loss of carbon dioxide as the concentra tion of hydrochloric acid began to drop. The carbon dioxide loss in mass over time was used to calculate the rate of reaction.In chemistry, the rate of reaction is used to describe how quickly a reaction happens. It is defined as the measure of the amount of reactants be converted into products per unit amount of time. In our case, we measured the amount of hydrochloric acid and calcium carbonate being converted into carbon dioxide in 20 seconds intervals. There are several(prenominal) ways to vary and experiment with a rate of reaction. Students can observe a change in volume of gas produced, change the transmission of light in the experiment, change the concentration using titration or even change the concentration using conductivity. For this experiment, we spy rate of reaction by a change of mass.We calculated our rate of reaction by dividing the grams of carbon dioxide released by 20 seconds. Because 20 seconds was a invariant divisor, the more mass of carbon dioxide release d, the greater the rate of reaction. We also calculated the concentration of HCl left and observed the relationship. Based on our processed data, the lower the concentration, the greater the rate of reaction. For example, after 320 seconds, 2.00 g of carbon dioxide was expelled when the concentration of HCl was 0.182 mol dm-3.This gives a rate of reaction of 0.1 g of carbon dioxide produced per second. At 20 seconds, 0.70 g of carbon dioxide was released when the concentration of HCl was a whopping 1.364 mol dm-3. This gave a rate of reaction of 0.035 g CO2 per second, which is 0.065 g more than the aforementioned low concentration. The two graphs confirm this conclusion. As time goes on, the mass of carbon dioxide expelled increases, plot of ground the concentration of hydrochloric acid decreases. A lower concentration of hydrochloric acid causes more carbon dioxide to be expelled and and so lead to a greater reaction rate.I was quite shocked by our results. I image that with a higher concentration and more molecules moving around, there would be a better destiny of reactions taking place. However, this experiment shows that it was in fact the other way around. Perhaps, with a lower concentration of hydrochloric acid, there needed to be more carbon dioxide expelled to balance out the comparison. With fewer moles of hydrochloric acid and lower concentrations, the equation was most likely out of proportion. In an attempt to make up for the lower number of moles, more carbon dioxide was released.LimitationSignificanceImprovementTearing of cotton wool when it was being removed from the flask and then losing the torn cotton.When the cotton wool was being removed, some it may conduct been torn off. As a result, the mass could be a lot lighter than it should have been. When taking out the cotton, vilify should be limited so that e verything is accounted for and a more accurate carbon dioxide mass is achieved.Be very careful when removing the cotton to avoid a ny tearing. If a piece of cotton is accidently torn off, do non throw it away Keep it and weigh it so that it is accounted for.Experiment was not performed until carbon dioxide stopped being expelled.The data was limited. Carbon dioxide was still being produced and there were still 0.091 moles of hydrochloric acid left when the experiment was stopped.Do not finish the experiment until there is no more carbon dioxide being expelled. This way, we get a better idea of the limits and possibilities of the reaction rate and how far it can go.Timer was not started the same time the marble was entered.Some marble could have been left inside the solution for a longer or shorter time than others. As a result, carbon dioxide values could be lower or higher than they should have been.The timer should be alert and there should be communication between the partners. The timer needs to bring down once the marble chips are placed inside, and it needs to be removed right after twenty seconds. By maintain a steady time of twenty seconds, we can properly assess the reaction rates without adding another independent variable of time.