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

Reaction Rate

Extracts from this document...


Science Reaction Rate Between an Acid and Metal Investigation PROBLEM/RESEARCH QUESTION In this investigation, a controlled experiment will be conducted to determine whether the varying concentration of an acid alters its reaction rate with a metal substance and if so, what is the resultant relationship between the rate of reaction and the concentration of the acid. In particular, we will be reacting Sulfuric acid (H2SO4) with Magnesium metal (Mg) and collect data based on the resultant hydrogen gas produced by the reaction. Word Equation: Magnesium + Sulfuric Acid ? Hydrogen gas + Magnesium Sulfate Balanced Equation: Mg (S) + H2SO4 (aq) ? MgSo4 (aq) + H2 (g) Research will be formulated by conducting a controlled experiment in which we will react 0.05g of Magnesium metal ribbons (Mg) with 10mL of four different H2SO4 (Sulfuric Acid) solutions varying in concentration and determine the time it takes for the reaction to produce 20mL of Hydrogen gas with each varying concentration. HYPOTHESIS I hypothesise that as the concentration of the H2SO4 solution increases/strengthens (measured in molarity mass), it will correspond to an increased/quicker rate of reaction with Mg metal. Hence, I also hypothesise that - based on the above premise- the 2M solution of H2SO4 would be the quickest to produce 20mL of H2 gas when reacted with magnesium, as it is the strongest of the four concentrations being trialed. My hypothesis is based upon the scientific reasoning that a more concentrated solution has more particles of the altering reactant (in this case H2SO4) present in a specific volume/amount of space than those present in a more dilute solution. Hence, at a higher concentration, particles are more likely to collide and react with one another, forming a larger number of new bonds between the two reactants. The ?Collision Theory? (which summaries the previous sentences) infers that the rate of reaction is impacted by how often molecules collide with one another. ...read more.


1. Measure out 10mL of the 0.5M, H2SO4 solution in second measuring cylinder and pour into large test tube. 1. (Start of trial) Place one strip of magnesium ribbon (0.05g) into large test tube and immediately cover top of tube with rubber stopper end of delivery tube. Ensure that it is firmly attached and air tight. As soon as reaction begins with H2SO4 solution already in test tube, start timing the rate of reaction using the stopwatch. 1. Measure and record the time it takes for the water level in the inverted measuring cylinder to decrease by 20mL. This will indicate that it has been replaced by 20mL of hydrogen gas. 1. Reset the experiment by rinsing the measuring cylinders and test tube with distilled water; refill the inverted measuring cylinder with 100mL of water and carefully place back into plastic container with delivery tube passing through it. 1. Measure another 10mL of 0.5M, H2SO4 solution in second measuring cylinder and pour into test tube. 1. Repeat steps 8 and 9 again, adding the 0.05g, Mg ribbon to the reaction in the test tube, cap of the test tube with the rubber stopper end of the delivery tube and time until 20mL of H2 gas has been produced in inverted measuring cylinder. 1. Rinse all equipment with distilled water once trial 2 is completed and measure out another 10mL of 0.5M, H2SO4 solution. Reset experiment like in step 10 and pour measured solution into clean test tube. 1. Begin trial 3 and repeat steps 8 and 10 again. If the previous two trials yielded similar results, trial 3 should also be of similar time length. If at the end of three trials, there is an anomaly within them, it may be required to complete a fourth trial to clean up data. 1. Repeat steps 7-14 again with the 1M, 1.5M and 2M H2SO4 solutions. ...read more.


we were interested in and hence were able to answer our research question in the affirmative that the concentration of an acid (in this Sulfuric acid) does effect its reaction of rate with magnesium metal, with the relationship being that an increase in concentration (molar mass) equates to an increased/quicker rate of reaction- evidenced by the time taken to produce 20mL of hydrogen gas. Our method was fairly clear, concise and allowed us collect our data in a fairly orderly way, doing so for most tests. It allowed us to complete the experiment with accuracy excluding the effects of the one, major problem (mentioned above) that were inevitable based on the way the experiment was conducted. Although our method and experimental plan were quite accurate, easy to understand and allowed us to achieve our target of determining a distinct and logical relationship, there are still many improvements that could be made to it to improve the validity of our results and further experiments could be carried out to extend this investigation. These include: * Completely eliminating human impact in the experiment by a valve of some sort to add the magnesium ribbons to the reaction in the test tube with the rubber stopper already firmly attached to the test tube. This will mean that the slight deviation in data is not experienced. * Using a larger sample size- (i.e. 8-10 different concentrations of H2SO4) so that the relationship gathered can be further strengthened and backed up by more evidence. * Investigate whether changing the concentration of H2SO4 has an impact on the time it takes for the reaction to reach equilibrium (the end of the reaction) and form a relationship from there. * Use different types of acids and metals with different properties to investigate if the rate of reaction is similar to that between Sulfuric acid and magnesium or it is quicker/slower. * Trialing different factors that affect the rate of reaction such as temperature or agitation and evaluating their influence compared to that of altering the concentration. ...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. Aim: Using an iodine clock reaction to find the order of hydrogen peroxide and ...

    Timer Error Somewhat Significant since the uncertainty of the time was carried forward to the rate, which gave a total uncertainty of 31% in the most extreme case. This is almost a 1/3, which means the time could have been 1/3 more or less, so the all experiments could have been more or less.

  2. Disappearing cross experiment

    beaker * While the water was heated up in the tea kettle the thermometer was put into the conical flask * The hot water was then poured into the beaker, without spilling anything into the conical flask * When the temperature of sodium thiosulphate was very close to the first and the lowest of the temperatures (22�C)

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

    Procedure: Part A: the effect of concentration on the rate of solvolysis of t - butyl chloride in 70%water - 30%acetone solvent. a- Experimental procedure: to measure the time necessary for 10 % solvolysis of t - butyl chloride (0.1 M concentration)

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

    The experiment is generally measuring the chemiluminescence of luminol, i.e. how long does it glow in these conditions? The dependent variable is time and the independent variables are concentration of luminol, concentration of hydrogen peroxide and temperature respectively. To develop fair tests, when investigating 1 of the independent variables, the remaining 2 have to remain constant.

  1. The purpose of this investigation is to determine the effect varying temperatures have on ...

    Create an observations table. Headings should include trial number, Temperature of HCl with uncertainty, Mass of Mg with uncertainty and Time taken for reaction to complete with uncertainty. Since there are 3 trials per condition and 5 conditions in total, there should be 15 trials listed in observations table. 5.

  2. Surface area vs Rate of Reaction

    could be treated with a shorter rubber tube so that it does not take as long for the gas to travel from the flask to the graduated glass tube When the rubber tube was submerged in water, water travels into the tube.

  1. Investigation of reversible reactions at equilibrium - CuCl2 (s) was added to HCl , ...

    According to Le chatelier?s principle when a system under equilibrium is stressed , the position of the equilibrium moves such that in order to oppose the stress .The position of the equilibrium moves to the lkeft in order to overcome this change in the concnetation and hence the color of

  2. Investigating Factors that Affect the Rate of Reaction of the Decomposition of Hydrogen ...

    Once the LoggerPro Program has been opened make sure that the label on the x-axis is time in seconds and that the units on the y-axis is pressure in kPa before collecting the data. Leave the test tubes in the water bath for at least two minutes so that the

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