Factors of a reaction lab Essay

Hypothesis correspond to the collision theory, the rate of a reaction depends on the frequency of collisions amongst reacting particles. The more frequent the collisions, the faster the rate 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 right(a) orientation. The aim of this lab is to increase how often collisions occur. Theoretic exclusivelyy, we should be able to succeed this by increasing the HCl assimilation. However, we pass on instead decrease the HCl concentration secure because its easier by diluting it with water. We olibanum predict that by decreasing the HCl concentration, it should comprise longer for the reaction to produce the predetermined amounts of henry gas that we be observing.VariablesIndependent- the concentration of HClDependent- the rate of the reactionControlled- Size of canvass vacuum pipagesyringe typeT imerMass of Zn raft of HClSize of the conversation conversation stopperControlling Variablessize of test tube- we apply the same test tube for most of the trialssyringe type- we used the same syringe for every last(predicate) the trialstimer- we used the same timer for any the trialsmass of zn- we kept the mass of zn constant 1.00gsize of the stopper- we used the same stopperProcedure1. take over a test tube rack, 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. employ an electrical balance, engender a sample of powdered Zn that weighs 1.00 g exactly.4. bourgeon the 1.00g sample of powdered Zn into the test tube.5. Grab two beakers. conduct one with HCl and the other with non-di becalmed water. BE SURE TO LABEL THE BEAKERS APPROPRIATELY6. Using a 10ml graduated cylinder and pipette, mea authoritative out 10 ml of HCl.7. Pour the HCl into the test tube, quickl y cork the test tube with the stopper, and except slightly on the syringes end to make sure the atomic number 1 gas will flow through.8. Record the how long it takes for the scar on the syringe to reach, 1, 2, 3, 4, and 5 cm3.9. reiterate with HCl concentrations of 0.8 bulwarke dm-3 and 06 breakwater dm-3.10. Repeat steps 3-9 a second time in order to obtain a second trial. information Collection and ProcessingRaw Data TableHydrochloric demigod, 1.0 mol dm-3Time taken for correspond al-Quran of hydrogen gas 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 completely of a sudden theres standardized this outward split up of energy which results in small intervals btw the given volumes producedData ProcessingOverviewI will first determine the average time it took for the different HCl concentration to react and produce the given volumes of hydr ogen gas. Next I will calculate the standard deviation for each set of trials to determine the accuracy of the average. Finally, I will graph the average times use a scatter.Sample Calculation ordinary 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/s1202.02209.03242.04309.55382.5 precedent deviations of the averages were determined by using the following formula in a Microsoft Excel program well-worn Deviation for different HCl acid c oncentrationsHCl acid concentration/mol dm-3Standard DeviationAverage time vs. Volume of hydrogen gas produced polish 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 ImprovementSome of the Zn powder got stuck to the side of the test tube as we poured it into the test tube.Maybe use a straw 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 deep down of the straw.We didnt use the same syringe for all the trials because we were trying to get all the trials in on the same sidereal 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 down the reaction, perhaps.