# Rate Of Reaction Lab Report

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Rate of Reaction Introduction: The Rate of Reaction defines the speed of the reaction that has taken place, determining whether it was fast or slow. For this experiment, I have decided to calculate the rate of reaction of the following equation: Hydrochloric Acid + Magnesium → Magnesium Chloride + Hydrogen 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) In order to increase the rate of reaction, these following factors needs to be put in mind: The Temperature The Concentration The Mass of a substance The Pressure (For Gases) A Catalyst can also increase the Rate of Reaction. Research Question: How does changing the concentration of 5 cm3 of Hydrochloric acid influence the rate of reaction wherein the rate of the reaction will be measured by the…show more content…
Procedure: Place Weighting Boat on Electronic Balance. (Ensure the Weighting Board has no contents and is dry and clean) Add 0.2 g of Magnesium Powder to the Weighting Boat on the Electronic Balance. (To ensure the amount is exactly 0.2 g) Transfer the 0.2 g of Magnesium Powder from the Weighting Boat to a 100 cm3 Conical Flask and seal the Conical Flask with a 2 holed rubber bung, connect one of the holes of the rubber bung with a 100 cm3 Gas Syringe. Measure 5 cm3 of Hydrochloric Acid using a 10 cm3 Plastic Syringe and place it on the other empty hole of the rubber bung. Once the Hydrochloric Acid from the Plastic Syringe is injected into the Conical Flask, start immediately start the Stop Watch. Once the Stop Watch reaches 20 seconds, calculate the volume of the Hydrogen Gas. (Trail 1) Reset the Gas Syringe back to Zero; then clean, dry and wash the Conical Flask to repeat the experiment two more times in order to gain the volume of Hydrogen Gas in order to get accurate results. (Trail 2 and Trail 3) Once 3 Trails has been completed, the entire experiment will be repeated with different concentrations of Hydrochloric acid (1.0, 1.5, 2.0, 2.5) with 3 Trails experimented for each…show more content…
Calculating the number of moles of Magnesium, Hydrochloric acid and Hydrochloric gas produced: Number of moles of Mg = mass/(molar mass) = (0.2 g)/24.31 = 0.0082 moles Concentration of HCl acid (mol/dm3) Volume of Hydrogen produced cm3 Number of moles of HCl ((emc ×volume)/1000) Number of moles of H2 moles of limiting reagent (reagent/(moles of H_2 )) 0.5 15.0 (0.5 ×5)/1000 = 0.0025 moles 0.0025/2 = 0.0013 moles 1.0 27.7 (1.0 ×5)/1000 = 0.0050 moles 0.0050/2 = 0.0025 moles 1.5 34.7 (1.5 ×5)/1000 = 0.0075 moles 0.0075/2 = 0.0038 moles 2.0 48.3 (2.0 ×5)/1000 = 0.0100 moles 0.0100/2 = 0.0050 moles 2.5 61.0 (2.5 ×5)/1000 = 0.0125 moles 0.0125/2 = 0.0063 moles Calculating theoretical yield, % yield and % error: Theoretical yield = number of moles x 24,000 % yield = (Experimental yield)/(Theoretical yield) x 100 % error = |(Experimental yield-Theoritical yield)/(Theoretical yield)| x 100 Concentration of HCl acid (mol/dm3) Volume of H2 produced (cm3) Number of moles of Hydrogen Theoretical yield (cm3) % yield % error 0.5 15.0 0.013 31.2000 48.0769% 51.9231% 1.0 27.7 0.0025 60.0000 46.1667% 53.8333% 1.5 34.7 0.0038 91.2000 38.0482% 61.9516% 2.0 48.3 0.0050 120.0000 40.2500% 59.7500% 2.5 61.0 00063 151.2000 40.3439% 59.6561% Calculating Rate of