Factors of a reaction lab Essay

HypothesisAccording to the collision theory, the place of a response depends on the frequency of collisions between reacting particles. The more rat the collisions, the speedy the tread of the reaction. However, in order for the collisions to be effective, the particles must collide with sufficient energy (activation energy). Furthermore, the particles must collide with the proper orientation. The aim of this lab is to increase how often collisions occur. Theoretic totallyy, we should be able to achieve this by change magnitude the HCl concentration. However, we cash in ones chips out instead decrease the HCl concentration just because its easier by diluting it with water. We thus predict that by decreasing the HCl concentration, it should take longer for the reaction to pass water the predetermined amounts of henry spatter that we are observing.VariablesIndependent- the concentration of HClDependent- the rate of the reactionControlled- Size of run thermionic pipeSyri nge type timerMass of ZnVolume of HClSize of the stopperControlling Variables coat of bear witness underground- we used the aforementioned(prenominal) canvass tube for most of the trials spray type- we used the same syringe for all the trialstimer- we used the same timer for all the trialsmass of zn- we kept the mass of zn constant 1.00g coat of the stopper- we used the same stopperProcedure1. Grab a test tube wedge, a test tube, a stopper that fits snuggly into the test tube and a syringe.2. Place the test tube into the test tube rack and attach the syringe to the test tube.3. Using an electric balance, obtain a sample of pulverise Zn that weighs 1.00 g exactly.4. Pour the 1.00g sample of milled Zn into the test tube.5. Grab two beakers. Fill one with HCl and the new(prenominal) with non-distilled water. BE SURE TO LABEL THE BEAKERS APPROPRIATELY6. Using a 10ml receive cylinder and pipette, measure out 10 ml of HCl.7. Pour the HCl into the test tube, quickly cork the test tube with the stopper, and pull slightly on the syringes end to dispatch sure the henry particle accelerator will flow through.8. Record the how long it takes for the marker on the syringe to reach, 1, 2, 3, 4, and 5 cm3.9. Repeat with HCl concentrations of 0.8 breakwater dm-3 and 06 mol dm-3.10. Repeat steps 3-9 a atomic number 42 time in order to obtain a second trial.Data Collection and ProcessingRaw Data TableHydrochloric mordant, 1.0 mol dm-3Time taken for corresponding volume of henry sport to be produced/sVolume of hydrogen gas produced/cm3Observations Zn clumps together at bottom of test tube Bubbles are produced No longer powder Nothing happens for a while and then all of a choppy theres like this outward burst of energy which results in small intervals btw the abandoned volumes producedData ProcessingOverviewI will depression determine the average time it took for the unalike HCl concentration to react and produce the given volumes of hydrogen gas. Next I wil l calculate the example deviation for each set of trials to determine the accuracy of the average. Finally, I will graph the average times using a scatter.Sample reckoning number of different trials for time taken for 1cm3 of hydrogen gas to be produced with 1.0 mol dm-3 of HCl(118 + 123)/2 = 120.5sHydrochloric acid, 1 mol dm-3Volume of hydrogen gas produced/cm3Average time taken for corresponding volume of hydrogen gas to be produced/s1120.52152.03190.54227.05274.0Hydrochloric acid, 0.8 mol dm-3Volume of hydrogen gas produced/cm3Average time taken for corresponding volume of hydrogen gas to be produced/s1137.02226.03330.04439.55552.5Hydrochloric acid, 0.6 mol dm-3Volume of hydrogen gas produced/cm3Average time taken for corresponding volume of hydrogen gas to be produced/s1202.02209.03242.04309.55382.5Standard deviations of the averages were determined by using the following convening in a Microsoft Excel programStandard Deviation for different HCl acid concentrationsHCl acid co ncentration/mol dm-3Standard DeviationAverage time vs. Volume of hydrogen gas produced shutting and EvaluationConclusion Hydrochloric acid, 1 mol dm-3 concentration, the highest concentration used in this experiment produced the given volumes of hydrogen gas the fastest out of all three HCl concentrations. Hydrochloric acid of 0.8 mol dm-3 concentration did produce 1 cm3 of hydrogen gas faster than hydrochloric acid of 0.6 mol dm-3 as predicted. Hydrochloric acid of 0.6 mol dm-3 concentration produced hydrogen gas faster than hydrogen gas of 0.8 mol dm-3.LimitationsSuggestions for Improvement virtually of the Zn powder got stuck to the side of the test tube as we poured it into the test tube.Maybe use a pale yellow or something like that to make sure the Zn gets to the bottom of the test tube. And like blow into the straw (softly) to ensure that none of the Zn gets stuck to the inside of the straw.We didnt use the same syringe for all the trials because we were trying to get all th e trials in on the same day.Use the same syringe for all trials.We didnt get all the trials in on the same day. I think it took us three classes. As a result, each day we were working in different room temperatures.Organize ourselves better so that we get all the trials in on the same day.We couldnt dry the test tube correctly. Each time we dried it there was still water at the bottom of the tube.Maybe like attach a paper towel to a stirrer and swap it around inside the test tube to dry it out.Zn is impure. As a result, the HCl acid could be reacting as well with whatever impurities present are thus slowing take the reaction, perhaps.