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

AimTo study the effects of ever-changing the move up body politic on the stray of a chemical responseHypothesisThis hypothesis is based on the Collision Theory, where in put together to oppose, the two particles involved must1. Collide with each other2. The collision must be energetic enough to overcome the activation slide fastener of the reaction3. The collision must bring the reactive parts of the blood corpuscle into contact the correct commission they must collide with appropriate geometry (the reactive parts)Considering that the excavate field of honor of a particle is a factor that in general affects the collision straddle of particles, it would be safe to assume that as the surface area increases, the reaction position increases.The graph should turn go forth to be something analogous this1. the reaction is the fastest at the start2. The reaction is diminish down here3. No to a greater extent product is formed measuring rod of product beatVariablesVariableF actorWhat is manipulatedDependentTimeThe metre it calculates for the reaction to complete supposes on the surface area of the conflates being apply, because it determines the rate in which the reaction leave occur.In symbioticVolume of the gas store (H2, CO2)The amount of gas accumulate for each experiment will depend on theControlled1. business deal of Calcium deoxycytidine monophosphateate (both marble chips and powdered form)2. Mass of atomic number 12 (both ornament and powder)3. Volume of Hydrochloric Acid4. Apparatus expenditured1. The the great unwashed of the amounts utilized will remain constantly fixed during the experiment2. 50 cm3 of HCl will be employ for every trial 550 cm3 in impart3. The apparatus used will remain the same throughout the tout ensemble experimentChemical ReactionsMg + 2HCl MgCl2 + H21. Magnesium ribbon2. Hydrogen louse up will be the gas collected1. 3 trials will count place1. Mass of Magnesium ribbon in1. Trial 1 0.064 grams2. T rial 2 0.063 grams3. Trial 3 0.065 gramsCaCO3 + 2HCl CaCl2 + H2O + CO21. marble Chips2. Carbon Dioxide will be the gas collected1. 2 Trials 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 c unmatched-shaped Flask (100cm3)5. 1 Single-holed rubber bung and delivery tube to salvo conical flask6. 1 Measuring cylinder (100cm3)7. StopwatchChemicals1. 12cm of Magnesium Ribbon2. 550 cm3 of Hydrochloric Acid3. Marble Chips4. Sodium Carbonate (Powdered)Method1. beat up apparatus as shown2. Fill the conical flask with 50cm3 of HCl3. confine the end of the syringe into the hole on top of the secure4. furnish the milligram ribbon5. Seal the flask with a r ubber stopper as quickly as you give notice, at the same epoch view as someone else present to start the stop watch once the magnesium ribbon has been added to the hydrochloric sour6. As the reaction takes place, note down the metre it takes for the gas collected to reach a multiple of 5 (i.e. 5mL, 10mL .50,55,60,65 etc)7. persist in measuring until the reaction has stopped, or you are unable to mea genuine any longer8. Repeat each experiment 3 times, upright to be sure the data collected is accurate9. At step 4, replace the underlined compound with the next compound after one experiment is completed data RecordedMagnesium Ribbon Mg + 2HCl MgCl2 + H2Trial 1 (0.064 0.005 grams)Time (in seconds) 0.05 sVolume (in cm3) 2.5 cm3ConclusionUnfortunately I was unable to hit a graph using time as the independent variable, because the laboratory that I had utilized did not make believe the equipment available to accurately to magnetic disk the data if time were to be the inde pendent variable. Another factor that contend into my decision was the fact that the sm on the wholeest calibration of the glass syringe I used was 5 cm3. Since the only visible cardments shown on the syringe were multiples of 5, it would only expect reasonable that I switch around the variables, making time the dependent variable, and the volume collected the independent variable, since I couldnt exactly measure how often 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 curve shows the reaction slowing down, but unluckily the curve continues. This is because the reaction is still taking place. I was unable to write down the rest of the data because the measuring tools that were available werent able to destroy to such a high degree. In some cases though, like in the powdere d sodium carbonate experiment, the reaction began so quickly that I wasnt able to eternize the time in most cases, so I just stuck with those that I had managed to note down. In other cases, in that respect 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 compare 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 diametric 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 chip s and powdered calcium carbonate. To my dis may I free-base 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, seeing as they have different outranks of responsiveness. These factors, including the concentration of the acid used, could in addition 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 problem with this experiment the elements positions in the reactivity series could have really 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. increase a substances surface area, like turning regretful 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. homogeneous thisOnly atoms on the surface can reactIf you break the substance down, moreatoms are exposed and ready to react.EvaluationConsidering the lack of real available, I think I was able to manage the experiment jolly 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 few 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 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. Studying 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 person would be watching the syringe rise and call out to record when ever 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 record 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 prey was to investigate whether or not different surface areas affected the rate of the reaction, I think that I have produced enough data to accommodate my theory.