• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

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

Extracts from this document...

Introduction

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.

Middle

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.

Conclusion

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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Investigate the rate of reaction of luminol in various factors. The objective was to ...

    Tangents of each concentration are drawn, the x and y values are obtained using ratio. Since there is error for 0.18M to 0.24M, so no tangents can be drawn for that 3 concentrations. The tangents represent the rate of reaction at different concentration.

  2. The rate of reaction between sodium thiosulfate and hydrochloric acid

    * Calculating the mean time taken for the cross to disappear: * Formula: Mean time taken = (1st + 2nd + 3rd experiment data) divided by 3 Concentration of sodium thiosulfate/ M Mean time taken for the cross to disappear (� 0.0100 seconds)

  1. Acids/Bases Design Lab. How does a change in the pH value of a solution ...

    (The solution was decanted into a waste beaker) The remaining zinc was then placed (with the use of tongs) in another clean, and dry 50cm3 beaker that was already massed, labeled 'Beaker ART1', in which it was washed with distilled water from distilled water bottle pumps.

  2. Enthalpy Change Design Lab (6/6)How does changing the initial temperature (19C, 25C, 35C, and ...

    as to ensure the level of agitation of the solution is consistent. Materials and Equipment: - 2 x Clean, dry, polystyrene cups - 2 x Temperature probe (+/- 0.3�C) - 2 x Vernier LabQuest interface wih Logger Pro data collection software - 1 x Electrically powered magnetic stirrer - 1

  1. In this experiment, the effect of concentration on rate of reaction was investigated. We ...

    This gives a rate of reaction of 0.1 g of carbon dioxide produced per second. At 20 seconds, 0.70 g of carbon dioxide was released when the concentration of HCl was a whopping 1.364 mol dm-3. This gave a rate of reaction of 0.035 g CO2 per second, which is 0.065 g more than the aforementioned low concentration.

  2. Chemistry extended essay - investigate the effect of 2-bromo-2-methyl propane concentration and temperature of ...

    hydrogen - bonding, 2- Cations are solvated by nucleophilic sites on water molecule (oxygen). And in this case of t-butyl carbonium ion the nucleophiles form strong covalent bond to carbon and converting the intermediate to a substitution product. The reaction mechanism is a sequential account of each transition state and

  1. Measuring the fatty acid percentage of the reused sunflower oil after numerous times of ...

    tables and calculations 21 ASLAN Özge Cemre D129077 Appendix 1: Calculations for Neutralization of Numerous Times Fried Sunflower Oil Samples: Calculations for sample 1 (5 times frying) : Trial 1: V = 71.5 ± 0.1 ml → Vε = 71.5 ± 0.1% ml m = 5.433 ± 0.001 g →

  2. Reaction Rate

    * The same climatic conditions present around the experiment. The climatic conditions, in particular temperature will remain the same throughout the experiment to prevent natural processes and disturbance from impacting the experiment. These will be kept the same as no windows will be opened or closed and the air conditioning will not change in temperature or switch on/off after the experiment has started.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work