The Effect of Concentration on the Rate of a Reaction
Aim- Our aim is to investigate the effect of concentration in the rate
of a reaction.
Method- Below is a step-by-step guide to exactly what we did to do the
experiment.
The first thing we did or we do in any experiment involving acid is
put on safety goggles so we do not ruin our eyes.
Ø We then went and gathered up the equipment to complete the
experiment. The list is below:
Ø A Balance (scales)
Ø A gas syringe (100 cm cubed)
Ø 3m Hydrochloric acid
Ø A conical flask.
Ø A clamp stand
Ø A Beaker
Ø A Measuring cylinder
Ø Three grams worth of marble chips
Ø Stopwatch
· We measured twenty millilitres of Hydrochloric acid in the measuring
cylinder we then poured the Hydrochloric acid into the conical flask.
· We then got a square piece of paper and then placed it on the
balance. We pressed the button with the T symbol on it; this then
turned the units to zero grams.
· We then got the tub of marble chips and measured out three grams of
marble chips.
· We then put the marble chips into the hydrochloric acid that we
poured into the conical flask, and then we quickly put the cork ,that
was on the end of the gas syringe, into the top of the conical flask.
· We then measured how many cubic centimetres were given off by the
reaction every ten seconds over a time span of one hundred seconds.
· The three grams of marble chips reacted too fast due to a grater
surface area being covered; therefore, we tried 1.5 grams worth of
marble chips.
· For the 1.5 molar acid experiment we did the same steps as above.
Below is a diagram of what we did…..
This is a table of a three molar acid, and how long it took for the
carbon dioxide to be produced.
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The Effect of Concentration of Acid on the Rate of Reaction With Calcium Carbonate Calcium + Hydrochloric ð Calcium + Carbon + Water Carbonate Acid Chloride Dioxide CaCO3 (s) + 2HCl (aq) ð CaCl2 (aq) + CO2 (g) + H2O (l) Introduction I will be using the reaction between calcium carbonate and hydrochloric acid to see how the concentration of acid affects the rate of a reaction. By doing the above experiment I will prove that the higher the concentration of acid, the faster a reaction will occur. I have carried out a previous experiment called the 'Disappearing Cross', in which I used the reaction between thiosulphate, hydrochloric acid and water to see how concentration affects the rate of reaction. When we added the hydrochloric acid to the water and thiosulphate a reaction occurred, causing the water to become foggy so that the cross was no longer visible through the conical flask. The results for the Disappearing Cross experiment were as follows; Volume of Thiosulphate (Cm3) Volume of Water (Cm3) Volume of HCl (Cm3) Concentration (%) Time taken for X to disappear (seconds) 5 25 5 17 711 10 20 5 33 286 15 15 5 50 185 20 10 5 67 113 25 5 5 83 82 You can see that when the hydrochloric acid was most dilute the cross took 711 seconds to disappear, and when the acid was most concentrated the cross took just 82 seconds to disappear.
A plastic pipette was cut so that it was shorter than the length of the test tube. The test tube was put in with the stem down, and that so the bulb was loosely sealed off the tube.
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