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

The aim was to become accustomed to working with the equipment and to find optimum levels of hydrochloric acid and magnesium ribbon to produce 60cm of hydrogen, a sensible amount to produce in the real experiment.

Extracts from this document...

Introduction

Aim: The aim was to become accustomed to working with the equipment and to find optimum levels of hydrochloric acid and magnesium ribbon to produce 60cm of hydrogen, a sensible amount to produce in the real experiment. We also began to investigate the effect of temperature on the rate and the result of the product (hydrogen). It also served to discover any errors in the procedure which could affect the final result and prevent us getting accurate results, thus allowing us to eliminate these errors in the real experiment. Diagram: Method: We attached a gas syringe via a plastic tube to a test tube and used a clamp and stand to hold the gas syringe in place. Having poured 25cm of hydrochloric acid (of strength 1M) into the test tube, we placed a strip of magnesium ribbon (which length varied each time we repeated the procedure) ...read more.

Middle

Amount of hydrogen gas produced (cm ) 2 39 3 44 3.5 45 4 56 4.5 63 Here are two tables showing the rate of the reaction between 25cm of hydrochloric acid and a 4.5cm strip of magnesium ribbon when the hydrochloric acid is heated to 40�C and 70�C respectively: Hydrochloric acid heated to 40�C Time (seconds) Volume of gas (cm ) 15 24 30 40 45 45 60 50 75 54 90 60 105 62 120 64 Hydrochloric acid heated to 70�C Time (seconds) Volume of gas (cm ) 15 25 30 39 45 50 60 58 75 62 90 64 105 64 120 64 Conclusion: In the first part of the pilot experiment, we discovered that the correct length of magnesium ribbon to produce approximately 60cm of hydrogen gas when allowed to react with 25cm of hydrochloric acid is 4.5cm. We also became aware of the products of the reaction, magnesium chloride and hydrogen gas. ...read more.

Conclusion

This is because the amount of hydrochloric acid and magnesium does not change, therefore the amount of magnesium chloride and hydrogen will not change, but because the temperature of the hydrochloric acid is higher, the atoms in the hydrochloric acid will be moving faster, and therefore will collide and bond (ionically) with the magnesium atoms quicker. We also discovered several points to remember in the second procedure to ensure accurate, reliable results. The hydrochloric acid was heated in a small beaker and this became very hot, so we had to use tongs to pour it into the test tube. As the reaction begins to happen even more quickly when the hydrochloric acid is heated, we had to ensure also that we were ready to immediately seal the test tube after pouring in the heated hydrochloric acid and placing the magnesium in immediately to avoid the hydrochloric acid cooling. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Physical 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 AS and A Level Physical Chemistry essays

  1. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    if concentration is measured in mol dm-3 and volume is measured in cm3. The total volume of the reacting mixture is 40cm3, so the actual concentration of X (in mol dm-3) is given by: (Equation 3.1.2) Putting together equations 3.1.1 and 3.1.2, we get the relationship: (Equation 3.1.3)

  2. Investigating how concentration affects rate of reaction

    Relating back to my theory section, this shows that the reaction, with respect to sulphuric acid, is second order. This in turn means that I have proved the final rate equation to be: Rate = k[BrO3][Br -][H+]2 This is exactly what I predicted at the beginning of my investigation.

  1. Describe the construction, operation and application of distillation equipment used in industry

    This is useful because as vapours and gases rise, some of them will condense when they pass through the liquid level on a tray at a certain temperature. Overall, it makes the distillation process a little bit more efficient as product can be collected more readily.

  2. Investigating the effect on the rate of reaction when changing the acid that is ...

    I have determined that they are strong and weak by studying their Ka values[3]. I tried to keep consistency between strong acids and also between weak acids with this value. We had a limited choice of acids but the ones I have chosen have the best consistency.

  1. The Determination of rate equation

    Justification for the Concentrations Used After watching the demonstration shown by the teacher, I noticed a cloudy solution forming within 14 seconds after mixing the 50cm� of (0.4 moldm-�) Na2S2O3 was mixed with 5.0 cm� HCL (2.0 moldm-�) diluted with 20cm� H2O.

  2. How do we make Magnesium and Hydrochloric acid react faster?

    A fixed amount of energy called activation energy (Ea) must be reached if the reaction is to take place. Particles need to collide with enough velocity so that they react. This means that they are colliding more often and more of the collisions have enough velocity and energy to cause a reaction.

  1. detremining the rate equation

    Volume of Na2S2O3 and HCl When changing the concentrations the volume will all so change. I will fill the rest of the volume with water to keep a constant overall volume to avoid a presence of another variable. Variables for method 1 Dependent variable - will be the time taken

  2. Does the amount of hydrogen gas formed in the below reaction depend on the ...

    Method: I will take my 30cm magnesium strip and divide it up into different lengths starting with 1cm, 2cm, 3cm, and 4cm. I will repeat this twice more using all of each length. One piece of each length was used in the preliminary investigation and the other two pieces of each length in the main experiment.

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