Rates of Reaction.

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Ross Bowman

Chemistry Coursework

Rates of Reaction

Introduction

This experiment was to determine the effect of changing one of the substrates when hydrochloric acid was mixed with calcium carbonate powder (chalk).  For this experiment, the variable was the concentration of the acid.

This was chosen in preference to calcium carbonate because it is difficult to determine particle size and subsequently measure an exact reaction, as smaller particles react quicker than larger particles.

The different concentrations of the hydrochloric acid were made up according to the following table:-

100cm3 2m acid + no water           =         2m

90cm3 2m acid + 10cm3 water =         1.8m

80cm3 2m acid + 20cm3 water  =         1.6m

70cm3 2m acid + 30cm3 water  =         1.4m

60cm3 2m acid + 40cm3 water  =        1.2m                m = moles

50cm3 2m acid + 50cm3 water  =        1m

40cm3 2m acid + 60cm3 water  =        0.8m

30cm3 2m acid + 70cm3 water  =        0.6m

20cm3 2m acid + 80cm3 water  =        0.4m

10cm3 2m acid + 90cm3 water  =        0.2m

The concentrations I chose were 2, 1.75, 1.5, 1 and 0.5moles.

Equation

The equation for this reaction is: –

Hydrochloric acid                                Calcium Chloride + water

                +                                        +

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Calcium carbonate                        Carbon Dioxide

2HCl (aq) + CaCo3 (s)                 CaCl2 (s) + H20 (l) + Co2 (g)

This will be an exothermic reaction as it will give out heat.

Equipment

Rubber bung

Plastic tubing

Conical flask

100ml plastic measuring cylinder

Plastic bowl

Stopwatch

Measuring beaker

Spatula

6-9mm particle size calcium carbonate

50 ml hydrochloric acid

China beehive

Top pan balance

Diagram


Method

  1. Set up the equipment as shown in the diagram.
  2. Weigh out 2.5g of calcium carbonate particles, 6-9mm.
  3. ...

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