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The Effect of Different Concentrations on the Rate of Reaction between Magnesium Ribbon and Hydrochloric Acid

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The Effect of Different Concentrations on the Rate of Reaction between Magnesium Ribbon and Hydrochloric Acid: Research Question: Does doubling the concentration of hydrochloric acid; double the rate of reactions when magnesium ribbon reacts with hydrochloric acid? Hypothesis: I believe that if we double the amount of hydrochloric acid concentration, the rate of reaction will also double. This maybe the case, because there is double the amount of particles reacting, hence, double the amount of collisions per second, causing double the amount of successful collision per second due to double the amount of kinetic energy. Hence, the reaction would finish in half the time. Independent Variable Dependent Variable Controlled Variable Concentration of hydrochloric acid- greater the amount of concentration, faster the rate of reaction. Volume of carbon dioxide gas produced in a certain amount of time- there must be a correlation between the acid concentration and the rate of reaction. ...read more.


1. Measure 50 cm3 of 1 mol dm-3 hydrochloric acid using a measuring cylinder. Pour HCL acid into the 100 cm3 conical flask. 2. Set up the apparatus as shown in the diagram above. 3. Then add a 15 cm strip of magnesium ribbon to the conical flask, immediately put the bung back into the flask as quickly as you can, and start the stopwatch. 4. Record the volume of hydrogen gas given off at suitable intervals (eg every 30 seconds). Continue timing until no more gas appears to be given off. 5. Repeat with different concentrations of HCL.( 1M, 2M, 4M) Results table: Acid Concentration- 1 mol/dm3 Time (seconds) Volume of Carbon dioxide gas given off (cm3) ((�0.5) 0 22 30 23 60 23 90 25 120 26 150 27 180 27 210 27 240 29 270 30 300 30 330 32 360 32 Average = 0.98 Acid Concentration- 2 mol/dm3 Time (seconds) Volume of Carbon dioxide gas given off (cm3) ...read more.


Evaluation: I was precise and accurate in my measurements as I measured the acid with a measuring cylinder to the line, viewing it at eye level. I used a ruler to measure the magnesium ribbon. I also used a large amount of volume of HCL to delete any temperature changes. * I should have repeated my experiment 3 times to have a greater significant difference between the three data's. * There were a few anomalous and big variations to my results table which could have been caused by escape of volume of carbon dioxide gas. Hence, I could improve the experiment by placing a shelf in the conical flask, for the magnesium ribbon, so no gas can escape. * I can also put the conical flask in a bath to make sure there is no temperature change. Hence, making my results more accurate. * I could put the magnesium ribbon in sand to get rid of any magnesium which has already reacted with oxygen, hence, weighing it to make sure they all have the same mass. ...read more.

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