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

Chemistry report - The aim of this practical is to observe the difference in the reactivity between Mg and Ca when hot and cold water is added.

Extracts from this document...

Introduction

Reactivity of Mg and Ca Introduction The aim of this practical is to observe the difference in the reactivity between Mg and Ca when hot and cold water is added. Hypothesis We think they will react in some kind of form. Variables The independent variable was the temperature of the water and also the quantity of metal use in the experiment and the dependent variable was the reaction. Equipment * Mg (s) * Ca (s) * Phenolphthalein * Beaker * Cold and hot water * Sandpaper * Test tubes with rack Procedure 1. ...read more.

Middle

5. Water was heated over a Benson burner and poured into the two test tubes without water while observing the reactions. 6. Two droplets of phenolphalein were added in each of the test tubes filled with cold water to observe the change in ph. Observation Relative reactivity of Cold water Hot water Mg There was a minimum reaction. Fig. 1 There is a bigger reaction than with the cold water. Fig. 2 Ca The temperature of the water increases right away. Before we dropped the phenolphthalein the solution was white, fig.3, but after adding the phenolphthalein it turned pink, fig.4, which means that the reaction is basic. ...read more.

Conclusion

In this case the atom that has more orbits is the calcium that is why it reacts more than the magnesium because calcium needs less energy to give electrons away. And the magnesium didn't react much because it needs more energy that the one that we gave it. Write the balanced equation for the reaction between Mg and H2O: Mg (s) + H2O (l) MgO (s) + H2 (g) Uncertainties Other element might have been present. The hot water might have been heated more. Conclusion We learned that both magnesium and calcium is basic solutions because of the pink tint to the color. We also learned that calcium reacted faster than magnesium. ?? ?? ?? ?? 10.11.11 nr.3 Inga and David ...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. Lab Report Reactivity

    1mo HCl: Iron: Initial temperature: 21�C � 1�C Final temperature: 23�C � 1�C Temperature change: 2�C � 1�C Aluminium: Initial temperature: 21�C � 1�C Final temperature: 21�C � 1�C Temperature change: 0�C � 1�C Copper: Initial temperature: 20�C � 1�C Final temperature: 21�C � 1�C Temperature change: 1�C � 1�C

  2. IB chemistry revision notes

    o They are the salt makers. o As we go down the group, atomic, ionic and covalent radii increase. Ionisation energies for this group are the second highest in the periodic table. o As we go down the group, the reactivity of the halogen decreases, but the halide's increases.

  1. Change of Potential Difference in Voltaic Cells Lab Report

    The different concentrations that we are going to use are: 0.2 M, 0.4 M, 0.6 M, 0.8 M and 1.0 M. Repeat these four steps for preparing the other concentrations of copper sulfate pentahydrate throughout the experiment. The different masses of CuSO4.5H2O for different concentrations can be calculated in the same way, using molar mass 249.71g/mol for CuSO4.5H2O.

  2. IB Chemistry Kinetics Exam Questions and Answers

    If the activation energy is lower, than more molecules will have the required activation energy and more collisions will be successful. 17. Determine the rate law for the following reaction A + 2B --> AB2 A (molarity) B (molarity) Rate (M/s)

  1. Determining the position of unknown element X in the Reactivity Series

    When ?E (?Energy) is +ve, the reaction taking place is endothermic and when ?E is -ve, the reaction will be exothermic. The reason behind the nature of ?H stated previously is the ?E (?Energy) of the reaction. Again; more the number of elements between the reactants (according to the Reactivity Series)

  2. Kinetics Practical

    12. Repeat the steps twice for two additional trials. 13. Repeat steps 1-3, however, this time use an ice bucket as an insulator. 14. Place about 8 ice cubes surrounding the solution beaker. 15. Using the stopwatch leave it for two minutes.

  1. Dissolved Oxygen in water

    This is to make sure that no air bubbles have been trapped inside, which would corrupt the reading. 8. Step 4: Invert several times the bottle. The sample becomes orange-yellow and a flocculent precipitate will form if oxygen is present.

  2. The chemistry of atmospheric and water pollution.

    Burning of biomass Note: Ozone is also formed in the lower atmosphere via photochemical smog. The nitrogen oxides in the photochemical smog absorb the U.V. radiation from sun and this produces an oxygen atom which then reacts with an oxygen molecule to produce ozone.

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