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1) The surface area of the magnesium.
2) The temperature of the reaction.
3) Concentration of the hydrochloric acid.
In the experiment we use hydrochloric acid which reacts with the
magnesium to form magnesium chloride. The hydrogen ions give
hydrochloric acid its acidic properties, so that all solutions of
hydrogen chloride and water have a sour taste; corrode active metals,
forming metal chlorides and hydrogen; turn litmus red; neutralise
alkalis; and react with salts of weak acids, forming chlorides and the
Magnesium, symbol Mg, silvery white metallic element that is
relatively unreactive. In group 2 (or IIa) of the periodic table,
magnesium is one of the alkaline earth metals. The atomic number of
Magnesium(s) + Hydrochloric acid(aq) = Magnesium Chloride(aq) +
In the reaction when the magnesium hits the acid when dropped in,
it fisses and then disappears giving of hydrogen as it fisses and it
leaves behind a solution of hydrogen chloride.
The activation energy of a particle is increased with heat. The
particles which have to have the activation energy are those particles
which are moving, in the case of magnesium and hydrochloric acid, it is
the hydrochloric acid particles which have to have the activation energy
because they are the ones that are moving and bombarding the magnesium
particles to produce magnesium chloride.
The rate at which all reactions happen are different. An example
of a fast reaction is an explosion, and an example of a slow reaction is
reactants chemical reactions® products.
We can measure reactions in two ways:
1) Continuous:- Start the experiment and watch it happen; you can use a
computer "logging" system to monitor it. I.e. Watching a colour fade or
2) Discontinuous:- Do the experiments and take readings/ samples from
the experiment at different times, then analyse the readings/samples to
see how many r…

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