Factors of a reaction lab Essay

HypothesisAccording to the collision theory, the score of a reaction depends on the frequence of collisions between reacting particles. The more frequent the collisions, the instant(prenominal) 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 befitting orientation. The aim of this lab is to increase how often collisions occur. Theoretically, we should be able to achieve this by increasing the HCl tautness. However, we will instead decrease the HCl concentration just because its easier by diluting it with peeing. We thus predict that by decreasing the HCl concentration, it should take longer for the reaction to produce the predetermined amounts of hydrogen bollix that we are observing.VariablesIndependent- the concentration of HClDependent- the rate of the reactionControlled- Size of shield resistanceSyringe typeTimerMass of Zn Volume of HClSize of the stopperControlling Variablessize of tally tobacco pipe- we used the resembling test tube for most of the trialssyringe type- we used the same syringe for all the trials ager- we used the same timer for all the trials flock of zn- we kept the mass of zn constant 1.00gsize of the stopper- we used the same stopperProcedure1. Grab 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. utilise an electric balance, obtain a sample of powdered Zn that weighs 1.00 g exactly.4. burgeon forth the 1.00g sample of powdered Zn into the test tube.5. Grab two beakers. execute one with HCl and the other with non-distilled water. BE SURE TO LABEL THE BEAKERS APPROPRIATELY6. Using a 10ml graduated 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 t he syringes end to make sure the hydrogen gas 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 mol dm-3 and 06 mol dm-3.10. Repeat steps 3-9 a countenance time in order to obtain a second trial.Data Collection and ProcessingRaw Data TableHydrochloric acid, 1.0 mol dm-3Time taken for corresponding volume 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 all of a sudden theres like this outwards burst 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 hydrogen gas. Next I will calculate the standard deviation for each set of trials to determine the accuracy of the av erage. Finally, I will graph the average times using a scatter.Sample CalculationAverage 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 measuring rod deviations of the averages were determined by using the following formula in a Microsoft Excel programStandard Deviation for different HCl acid concentrationsHCl acid concentration/mol dm-3Standard DeviationAverage time vs. Volume of hydrogen gas producedCon clusion and EvaluationConclusion Hydrochloric acid, 1 mol dm-3 concentration, the highest concentration used in this prove 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 inside of the straw.We didnt use the same syringe for all the trials because we were onerous to get all the trials in on the same day.Use the same syringe for all trials.We didnt get all the trials in on the s ame 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.