Effect of Changing Concentration on the Order of Reaction

Effect of Changing absorption on the Order of responseTitle An Investigation into the Effect of Changing the Concentration by Continuous Method on the Order of ReactionPlanningA. HypothesesI predict that the lay of reaction is influenced by the tautness of the reactants and that the position of reaction and the ducking of reactants decrease as time intervals increase. I predict that the order of reaction is affected or influenced by the parsimony of the reactant. I also predict that the change in concentration of reactants affects the rate of reaction proportionately and hence, the order of reaction. Such that, if the concentration of the reactants is reduce by half, the rate of reaction go away also decrease by a certain proportion.The reaction that will be analyzed in this sample is between a metal (magnesium ribbon) and an window glass (sulfuric acid). The reaction is shown by the chemical substance equation belowMg (s) + H2S04 (aq) MgS04 (aq) + H2 (g)In this experim ent, 0.15 grams of magnesium ribbon will be utilise in additional, together with 10 cubic centimeters of 0.3 M sulphuric acid (H2SO4). The continuous method will be used, where the metal is in excess and the reaction goes to completion. The glitz of the atomic number 1 flatulency (H2) will be self-possessed at a measured time interval of 30 seconds. These volume readings at the time intervals shall be recorded and analyzed.III. BackgroundThe rate of a reaction depends in part on the concentrations of the reactants. The rate at which a reactant or reactants is alter into products is the change in concentration of the reactant or reactants with time, (Wilbraham, et.al., 1997). Mathematically, the rate shag be expressed as drift = Change in Concentration of Reactants / Change in timeThe formula implies that the rate of disappearance of the reactants is proportional to its molar concentration. HenceChange in Concentration of Reactants / Change in time = proportional to the conce ntration of reactantsThe reaction rate has to be experimentally determined. From the reaction rate equation, the order of reaction can be obtained. The order of reactions can be classified as cryptograph order, first order, or second order, with respect to only one reactant.IV. Risk AssessmentIn this experiment, sulphuric acid (H2SO4), will be used as a reactant. Since it is a strong acid and is in truth corrosive, I will observe the following precautionary measuresWear protective goggles for the eyes. bar pipetting the sulphuric acid by mouth.Avoid inhalation of sulfuric acid.Care in handling the acid should be observed. It should be prevented from being knocked over.V. Fair running gameTo ensure that the results that I will obtain in the experiment are reliable and accurate, I will observe the followingThe volume measurements of the sulphuric acid reactant will be made very accurately by reading from the lower meniscus of the 10 cubic centimeter markThe bung will be securely and tightly placed to prevent the collected hydrogen blow out (H2) from escaping.The weight measurements of the magnesium ribbon will be made very accurately.All materials will be soundly cleaned before each use in order to prevent contamination.The experiment will have 3 runs or replicates in order to attain a high reliability of results.VI. Procedure of the ExperimentMaterials neededStopwatch for time interval measurements100 cc gas syringe for the Hydrogen gas collection100 cc conical flask for the sulphuric acid100 ml graduated cylinder for mensuration the sulphuric acidAnalytical balance for measuring 0.15 grams of magnesium ribbonProcedure1. Set up the materials sequence making sure that they are thoroughly clean and dry.2. Using a graduated cylinder, measure 10 cc of 0.3 Molar concentration of sulphuric acid.3. Carefully weigh 0.15 grams of magnesium ribbon victimization an analytical balance to make sure that the weight measurement is accurate.5. Put the 0.15 grams of magne sium ribbon into the conical flask with the sulphuric acid.7. Measure the volume in cubic centimeters of hydrogen gas collected in the gas syringe at any time interval of 30 seconds.8. Record the volume of collected hydrogen gas at each set time interval.9. Make 2 more runs of this experiment by repeating steps 1-8 at every run.VII. Results.Below are the tabulated volume measurements at every time interval circumvent 1 chroma Measurements for Run 1The data in card 1 were plotted in a graph belowGraph 1 Volume vs. Time (Run1)For Run 2, the data were obtained were tabulated belowTable 2 Volume Measurements for Run 2The data in Table 2 were plotted in a graph belowGraph 2 Volume vs. Time (Run 2)For Run 3, the data were obtained were tabulated belowTable 3 Volume Measurements for Run 3The data in Table 3 were plotted in a graph belowGraph 3 Volume vs. Time (Run3)All three graphs show the cut off that as time increases, the volume of the reactant decreases, while the volume of the pr oduct increases.B. Calculation of the Concentration of ReactantFrom the reactionMg (s) + H2SO4 (aq) MgSO4 (aq) + H2 (aq)Concentration is measured in terms of Molarity, where Molarity is equal to the number of moles of solute divided by liters of solutionMolarity = No. of moles of solute / Liters of solutionFor Magnesium (Mg), 0.15 grams were added to sulphuric acid. The number of moles is equal to weight in grams divided by the formula weight. Hence, the number of moles = wt. in grams / FW. Since 0.15 grams were used, 0.15 grams should be divided by the formula weight of Magnesium (Mg), which is 24.So 0.15 grams / 24 = 0.00625 moles for Mg.To get the molar concentration, the number of moles will be divided by the volume of the solution in liters, which is 0.01.So, the molarity of Mg is 0.00625 / 0.01 = 0.625 MFor the sulphuric acid (H2SO4) used, the molarity is 0.3 M. The number of moles of H2SO4 used is determined by multiplying the molar concentration by the volume of solution i n liters. Hence 0.3 moles/L X 0.01L = 0.003 moles.From the chemical equation of the reaction, for every 0.003 moles of H2SO4 used, the same amount of moles (0.003) of hydrogen gas (H2) is effrontery off.The molar concentration of the hydrogen gas evolved can now be determined for each respective time interval, by dividing the number of moles by the volume obtained.For run 1The concentration of the product can now be calculated, using the formula for reaction rate, where Molarity = Number of moles / Liters of solutionThe data for the concentration of the hydrogen gas are tabulated belowTable 4 Molarity of the hydrogen gas (H2)The molarity values tabulated above are plotted in the graph belowGraph 4 Concentration vs. Time (Run1)Graph 5 Concentration vs. Time (Run 1) Showing the Gradient of the Tangent CurveThe rate of reaction was calculated by measuring the gradient of the tangent of the curve above, as depicted by the red line. Hence, the gradient of the tangent is equal to 0.12 0 .05 / one hundred fifty = 0.00046. From the rate equation, the rate constant (k) can be obtained by the formula k = rate x H2SO4. So k = (0.00046) / 0.3 = 0.153. The rate equation is stride = k H2SO4Rate = (0.153) (0.003) = 0. 000459 or 0.0046. Hence, this value is equal to the gradient of the tangent of the graph above. This shows that the rate is directly proportional to the concentration of the sulphuric acid (H2SO4).Table 5 Concentration of Gas Collected and Rate of Reaction (Run 1)The plotting of tabulated data above results to the graph belowGraph 6 Rate vs. Concentration (Run 1)The Rate Concentration Graph for Run 1 above shows that the concentration of hydrogen gas (H2) is directly proportional to the rate of reaction. Thus, the concentration of sulphuric acid (H2SO4) is also directly proportional to the rate of reaction, whereby, as the concentration decreases, the rate of reaction also decreases.Since the Magnesium ribbon is in excess, only the sulfuric acid can be allowe d to change. Having it in excess is to make sure that its concentration does not change.Using the rate of reactionRate = k H2SO4And applying the rate equation to the chemical equation in the reactionMg (s) + H2SO4 (aq) MgSO4 (aq) + H2 (g)The rate equation is now Rate = k Mg H2SO4.Since Mg concentration does not change in the reaction, it is the zero order. On the other hand, since H2SO4 is in the first order of reaction, the rate is directly proportional to its concentration, as measured in the experiment by the concentration of the H2 gas collected, the overall order of reaction is 0+1 = 1.For Run 2, the table below shows its concentration.Table 6 Molarity of the Hydrogen gas (Run2)The table of Concentration and Time for run 2 gives the following graphGraph7 Concentration vs. Time (Run 2)The Concentration Time Graph for run 2 above shows the same trend as in run 1, where it shows an inverse proportionality as time increases, the concentration of the sulfuric acid ( H2SO4) decreas es as measured by the concentration of the hydrogen gas (H2) collected. The rate of re