Investigating the Effects of Surface Area on the Rate of Reaction Essay

AimTo study the make of changing the cake realm on the rate of a chemical reactionHypothesisThis hypothesis is based on the bang Theory, w here in order to react, the two particles involved must1. Collide with for each peerless other2. The collision must be energetic enough to overcome the activation energy of the reaction3. The collision must go the unstable parts of the molecule into contact the correct way they must collide with appropriate geometry (the reactive parts)Considering that the rear area of a particle is a concomitantor that mainly affects the collision rate of particles, it would be safe to assume that as the summon area increases, the reaction rate increases.The graph should turn emerge to be something like this1. the reaction is the fastest at the start2. The reaction is slowing down here3. No more than(prenominal) product is formedAmount of productTimeVariablesVariableFactorWhat is manipulated unfreeTimeThe season it takes for the reaction to compl ete depends on the surface area of the compounds being used, because it determines the rate in which the reaction will occur.IndependentVolume of the bumble roll up (H2, CO2)The amount of feature imperturbable for each experiment will depend on theControlled1. plurality of Calcium Carbonate (both marble chips and powdered form)2. Mass of Magnesium (both ribbon and powder)3. Volume of Hydrochloric Acid4. Apparatus purposed1. The masses of the substances utilized will die hard constantly fixed during the experiment2. 50 cm3 of HCl will be used for every trial 550 cm3 in total3. The apparatus used will remain the resembling throughout the whole experiment chemical ReactionsMg + 2HCl MgCl2 + H21. Magnesium ribbon2. Hydrogen Gas will be the gas collected1. 3 examinations will take place1. Mass of Magnesium ribbon in1. Trial 1 0.064 grams2. Trial 2 0.063 grams3. Trial 3 0.065 gramsCaCO3 + 2HCl CaCl2 + H2O + CO21. Marble Chips2. Carbon Dioxide will be the gas collected1. 2 Tria ls will take place1. Mass of Marble Chips in1. Trial 1 3.998 grams2. Trial 2 3.988 gramsNa2CO3 + 2HCl 2NaCl + H2O + CO21. Sodium Carbonate (Powdered)2. Carbon Dioxide will be the gas collected1. 2 Trials will take place1. Mass of Sodium Carbonate1. Trial 1 0.504 grams2. Trial 2 0.505 gramsApparatus1. Eye-Protection 1 pair of Safety Glasses2. 1 pair of scissors3. 1 Electronic Scale4. 1 Conical Flask (100cm3)5. 1 Single-holed rubber bung and livery tube to fit conical flask6. 1 Measuring cylinder (100cm3)7. StopwatchChemicals1. 12cm of Magnesium thread2. 550 cm3 of Hydrochloric Acid3. Marble Chips4. Sodium Carbonate (Powdered)Method1. Set up apparatus as shown2. binge the conical flask with 50cm3 of HCl3. Insert the end of the spray into the hole on top of the stopper4. add up the magnesium ribbon5. Seal the flask with a rubber stopper as quickly as you nates, at the alike(p) time cast someone else present to start the stop watch erst the magnesium ribbon has been added to the hydrochloric acid6. As the reaction takes place, note down the time it takes for the gas collected to reach a multiple of 5 (i.e. 5mL, 10mL .50,55,60,65 etc)7. Keep measuring until the reaction has stopped, or you are unavailing to measure anymore8. Repeat each experiment 3 times, just to be sure the entropy collected is accurate9. At step 4, deputize the underlined compound with the next compound after one experiment is completedConclusionUnfortunately I was unable to create a graph employ time as the independent variable, because the research laboratory that I had utilized did not have the equipment available to accurately to disk the information if time were to be the independent variable. Another factor that played into my decision was the fact that the smallest calibration of the glass syringe I used was 5 cm3. Since the altogether visible measurements shown on the syringe were multiples of 5, it would only seem reasonable that I switch around the variables, making time the dependent variable, and the brashness collected the independent variable, since I couldnt exactly measure how much gas would be collected every 5 seconds otherwise the relationship the graph would depict would be completely incorrect.As you can see on the graphs, the slightly steep slopes show when the reaction is the quickest, as it should be in the beginning. The switch off shows the reaction slowing down, but unfortunately the curve continues. This is because the reaction is still taking place. I was unable to record the rest of the data because the measuring tools that were available werent able to record to such a high degree. In some cases though, like in the powdered atomic number 11 carbonate experiment, the reaction began so quickly that I wasnt able to record the time in most cases, so I just stuck with those that I had managed to note down. In other cases, there were so many distractions in the lab that it was difficult to remain focused. My classmates kept re moving some if the items that I was victimisation.The idea was to see how the rate of reaction changed when the surface area of a substance was increased. Initially, my plan was to react magnesium ribbon and magnesium powder with 1 mole of Hydrochloric acid so I could compare and contrast how the surface area of the substance touch the rate of reaction. I had planned to keep everything about the two substances the same. Its portion, mass, the amount of Hydrochloric acid I was discharge to react with it the only thing unlike would be its surface area. Unfortunately the Lab didnt have any available. So I decided to do the same experiment to Calcium Carbonate, this time using marble chips and powdered calcium carbonate. To my dismay I found that the powdered calcium carbonate wasnt reacting at all. So I had to change it to sodium carbonate.There is skepticism about using different fractions, seeing as they have different orders of reactivity. These factors, including the concentra tion of the acid used, could also affect the rate of reaction. However, the same acid concentration was used for all experiments, in all trials so we can dismiss that. However, sodium is much higher up the reactivity series than calcium, which is higher up the reactivity series than magnesium. This is the riddle with this experiment the elements positions in the reactivity series could have really altered the rate of reaction.However, the experiments still settle that when the surface area of a substance is increased, the rate of reaction increases as well. This happens because, when two substances react only the surface particles of the substances can come into direct contact with the reactant particles. Increasing a substances surface area, like turning big solid chunks of calcium carbonate into powder, leaves more solid particles available to react. The more particles available to react at one time, the faster the rate of the reaction.Like thisOnly atoms on the surface can reac tIf you break the substance down, moreatoms are exposed and ready to react.EvaluationConsidering the overleap of material available, I think I was able to manage the experiment fairly enough to give away results. However, I am not pleased with the factors that may or may not have change my results, and the circumstances in which I had to switch my variables around. Therefore I would like to state a a few(prenominal) things I would like to alter, if ever I got the change to do this experiment again.1. Apparatus1. Next time, alternatively of using a stopwatch, I would like to use a digital device, like a laptop computer for example, that was somehow connected to the glass syringe, which was programmed to record the volume of the gas collected every 5 seconds. This time the graph would turn out the way it should be.2. Instead of using a measuring cylinder, I would replace it with a burette, as it takes more accurate measurements of liquids.1. Chemicals Used1. I would try and used the same element next time the only difference would be the surface area. For example, if I used magnesium, to study the effects of surface area on the rate of reaction, I would only you magnesium ribbon and magnesium powder. analyse different elements with different reactivitys would dismiss any data already collected because an elements position on the reactivity series may also determine the rate of reaction. Use the same element.1. Amount of People involved in the experiment1. If I had to do the experiment again, with the same apparatus, I think I would like to have 3 people participating in the appealingness of data. 1 person would be watching the syringe rise and call out to record whenever it rose, the second person would time it, and the 3rd person would record it. This time, the data may be even more accurate, because no one is taking their eye off the experiment, like I was doing during my experiment just to record data.I feel that altering these aspects of the experimen t would increase the level of accuracy, as to get more material data to calculate the order of reaction. Unfortunately with the data I have so far, I am unable to derive the concentrations of the substances I had utilized in my experiment. However, as the objective was to investigate whether or not different surface areas affected the rate of the reaction, I think that I have produced enough data to support my theory.