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

AimTo tuition the effects of changing the rebel sphere on the rate of a chemical reactionHypothesisThis hypothesis is based on the collision Theory, where in order to react, the two particles involved must1. Collide with separately other2. The collision must be energetic decorous to overhaul the activation energy of the reaction3. The collision must bring the unstable parts of the molecule into contact the correct way they must clash with appropriate geometry (the reactive parts)Considering that the protrude land of a particle is a factor that mainly fixs the collision rate of particles, it would be safe to give birth that as the surface area increases, the reaction rate increases.The graph should acquire out to be close tothing wish well this1. the reaction is the fastest at the swallow2. The reaction is slowing down here3. No to a greater extent produce is formedAmount of productTimeVariablesVariableFactorWhat is manipulated unfreeTimeThe time it takes for the rea ction to complete depends on the surface area of the compounds being used, because it determines the rate in which the reaction will occur.Independent masses of the gas store (H2, CO2)The amount of gas collected for each try out will depend on theControlled1. Mass of Calcium transform (both marble chips and powdery form)2. Mass of Magnesium (both palm tree and powder)3. Volume of Hydrochloric Acid4. setup Used1. The masses of the substances utilized will remain constantly placed during the essay2. 50 cm3 of HCl will be used for every tally 550 cm3 in total3. The apparatus used will remain the self self resembling(prenominal)(prenominal) throughout the whole tasteChemical ReactionsMg + 2HCl MgCl2 + H21. Magnesium ribbon2. Hydrogen Gas will be the gas collected1. 3 tribulations 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 + water + CO21. Marble Chips2. Carbon Dioxide will be the gas co llected1. 2 Trials will take place1. Mass of Marble Chips in1. Trial 1 3.998 grams2. Trial 2 3.988 gramsNa2CO3 + 2HCl 2NaCl + H2O + CO21. atomic number 11 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 condom Glasses2. 1 pair of Scissors3. 1 Electronic home base4. 1 Conical Flask (100cm3)5. 1 Single-holed rubber bung and rescue tube to fit conical flask6. 1 Measuring piston chamber (100cm3)7. S apex play alongChemicals1. 12cm of Magnesium Ribbon2. 550 cm3 of Hydrochloric Acid3. Marble Chips4. Sodium Carbonate (Powdered)Method1. Set up apparatus as shown2. Fill the conical flask with 50cm3 of HCl3. Insert the end of the syringe into the hole on top of the stopper4. Add the atomic number 12 ribbon5. Seal the flask with a rubber stopper as quickly as you can, at the similar time lose someone else present to start the stop watch once the magnesium ribbon has been added to the hydrochloric acid6. As the reaction takes place, pit down the time it takes for the gas collected to reach a treble of 5 (i.e. 5mL, 10mL .50,55,60,65 etc)7. Keep measuring until the reaction has stopped, or you are ineffective to measure anymore8. Repeat each experiment 3 times, vindicatory to be sure the info collected is accurate9. At whole step 4, replace the underlined compound with the next compound after one experiment is completedConclusionregrettably I was unable(p) to create a graph exploitation time as the independent variable, because the lab that I had utilized did not have the equipment useable to accurately to eternise the info if time were to be the independent variable. Another factor that played into my ratiocination was the fact that the smallest calibration of the glass syringe I used was 5 cm3. Since the save visible measurements shown on the syringe were multiples of 5, it would only retrievem commons ensical that I switch around the variables, making time the dependent variable, and the intensiveness collected the independent variable, since I couldnt exactly measure how much(prenominal) gas would be collected every 5 seconds otherwise the kin 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 edit out shows the reaction slowing down, but unfortunately the curve continues. This is because the reaction is still victorious place. I was unable to magnetic disk the rilievo of the entropy because the measuring tools that were available werent able to record to such a high degree. In some cases though, like in the fine-grained sodium 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 removing some if the items that I was using.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 contrast and contrast how the surface area of the substance affected the rate of reaction. I had planned to keep everything about the two substances the same. Its element, mass, the amount of Hydrochloric acid I was going to react with it the only thing different 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 elements, beholding as they have di fferent orders of responsiveness. These factors, including the concentration 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 high up the reactivity series than calcium, which is higher up the reactivity series than magnesium. This is the problem with this experiment the elements positions in the reactivity series could have rightfully altered the rate of reaction.However, the experiments still prove 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 hearty chunks of calcium carbonate into powder, leaves more solid particles available to react. The more particles available to react at one time, th e faster the rate of the reaction.Like this yet atoms on the surface can reactIf you break the substance down, moreatoms are exposed and ready to react.EvaluationConsidering the lack of material available, I think I was able to manage the experiment fairly enough to produce results. However, I am not pleased with the factors that may or may not have affected my results, and the circumstances in which I had to switch my variables around. Therefore I would like to state a a couple of(prenominal) things I would like to alter, if ever I got the change to do this experiment again.1. Apparatus1. Next time, instead of using a stopwatch, I would like to use a digital device, like a laptop for example, that was in some way 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. sort of 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. poring over 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 collection of data. 1 soul would be watching the syringe rise and call out to record whenever it rose, the 2nd 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 r ecord data.I feel that altering these aspects of the experiment would increase the level of accuracy, as to get more substantial 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 check into whether or not different surface areas affected the rate of the reaction, I think that I have produced enough data to support my theory.