Rates of Reaction Lab Investigation

Chemestry Lab Rates of Reaction (Picture from http//sciencespot. wampum/Pages/kdzchem. html) The pass judgment of reception is how fast or slow a response is completed. This is important for factories and chemists all all over the world. What happenes during a chemical reaction is atoms or molecules that shake up and convention new molecules. You can affect this rate of reaction with temperature of reactants or suroundings, surface bea of reactants, if there is a catalyst present, but in theis lab the closeness was metamorphosed as the IV. The reaction rate is masured in agitate/time, in this case it was loudness of hitmanolenes produced/minutes. bollix up was measured in ml/minute, and this was the DV. work out of lab was To find the change in rate if reaction, depending on the ducking of hydrocloric acid. Hypothesis If the concentration of hydrocloric acid is attachd, the rate of reaction will increase and the volume of gass will increase. The reasoning behind the hypothesis is that when there are more than than molecules in the solution the reactants collide more often, so more product is made in a shorter hitche of time. The equation was Mg + 2HCl MgCl2 + H2 akin article Measuring Reaction Rate Using Volume of Gas ProducedIndependent variable Dependent variable Controled variables Value How to control the CV compactness of acid Rate of reaction Vol of acid 20 ml handbill using a 50ml Measuring cylinder 2 moles pr. L Vol of gas Temp of acid Room temp. Not controlled, only montored 1 moles pr. L Amount of Mg 5 cm or ornamentation/ 0. 07g Ruler, and tilt 0. 5 moles pr. L Precence of catalyst No Not have a catalyst 0. 25 moles pr. L Type of acid Hydrocloric Have alike type of acid Method 1. Gather aparatus and materials, and set up as shown in diagram below aparatus list. 2. Bucket + pissing 3. Measure temp, in room and water 4.Fill measuring cylinder with water 5. dick furnish + sidearmed test tube 6. Obtain 0. 08 g using a w eight, straddle in side-armed test tube 7. 20 ml HCl of 2 moles pr. L in measuring cylinder 8. Place measuring cylinder in bucket with water, upside down, without air leaking in to the cylinder when flipped. 9. Puor HCl into side-armed testtube. 10. Start the stop watch 11. Close the top of the side-armed test tube by placing rubber knock 12. Weight 3 min. be accurate using the stopwatch 13. land ml of gas produced 14. Reapeat the look into twise pr. Concentration 2 moles pr L, 1 mole pr. L, 0. 5 moles pr. L and 0. 25 moles pr. L Aparatus list Sidearemd testtube Rubber plug Rubber tube Bucket Water 2x 100ml measuring cylinder 400ml Beaker 40 ml in each concentration type of HCl acid, 2, 1, 0. 5 and 0. 25 M. Pr. L 8x 0. 08g of Mg bay wreath Stopwatch Raw entropy dining table presentation amount of gas created in the two trials of the experiment Concentration in moles pr. L Trial 1 ml og gass produced in 3 min Trial 2 ml og gass produced in 3 min 0. 25 8 10 0. 50 3 0 32 1. 00 70 73 2. 00 61 65 First proceced data table showing average of gas made Concentration in moles pr. L Average of trial 1 and 2 in ml of gas produced in 3 min 0. 25 9 0. 50 31 1. 0 71. 5 2. 00 63 Proceced data table showing rate of reaction Formula used=ml of gass produced/time (in seconds) Concentration in moles pr. L Rate of reaction calculation in ml/sec Rate of reaction result in ml/sec 0. 25 9/180 0. 05 0. 50 31/180 0. 17 1. 00 71. 5/180 0. 40 2. 00 63/180 0. 35 Graph showing the rate of reaction Conclusion As the results clearly show, the rate of reaction increases rapidly and this strongly supports my hypothesis. The amount of succesfull collisions increased, because of increased number of atoms in the product, so when the concentration was increased it rate of reaction increases.There are more collisions because of more atomes, and therefor more succesfull once. Evaluation Random errors * Therometer used to measure temperature * Inaccuracy of +/- 1 C * Balance weig ht used to measure Mg ribbon * Inaccuracy of +/- 0. 01 g * Measuring cylinders used to measure volume of acid and volume of gas * Inaccuracy of +/- 0. 5 ml * Ruler used to measure Mg ribbon * Inaccuracy of +/- 0. 1 cm Ways to maintain random errors and amend the method Compleet the experiment more times Systematic errors As you adjoin in the graph, the fourth result was anomalus.During the 3 minutes the magnesium ribbon was used up in a very short period of time. The rate was so fast in the 2 moles per liter that it was over in under a minutte, but in the early(a) concentration types it tok longer time for the reaction to compleet. Therefor we have to look remote from the highest concentrations, and focus on the three lowest. This was a big weakness in the lab. When pouring the HCl acid into the side armed test tube, some of the reaction had been compleeted before we had time to put the rubber stopper on all(prenominal) time. The temperature was only monitored, not controll ed. Ways to reduce systematic errors and improve the lab * Have a shorter reaction time shorten the time form 3 min to around 1 minutte. * Use a fisle-funnle to prevent gas leaking out before the stopper is placed on the testtube. * Do the experiment in a controlled environment, like in a water bath. Sugestions to possible further investigations into this topic You can change the IV, to one of the other factors that affect rate of reaction. Eg. Take the same concentration of HCl acid and change the temperature, or the precence of catalyst.