acid rain course wrk

basically its wt i did for my gcses course wrk for core science. might find it helpful to get clues frm  it since i gt 13/16 pretty gd for reference.

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JOAN NSIMBI
AIM; TO INVESTIGATE THE RATE OF CARBON DIOXIDE PRODUCTION WITH VARYING CONCENTRATION
OF HCL ON CALCIUM CARBONATE.
INTRODUCTION;
In this experiment, I will use calcium carbonate in form of marble chips and hydrochloric acid since
when hydrochloric acid and the calcium carbonate are put together, they react. The products in this
reaction are carbon dioxide, water and calcium chloride. This experiment is going to suit my aim since
there is production of the carbon dioxide during the reaction.
Chemical equation;
Hydrochloric acid + calcium carbonate calcium chloride + carbon dioxide + water.
Equation in chemical symbols;
HCl (aq) + CaCO3(s) CaCl2 (aq) + CO2 (g) + H2O(l)
PREDICTION
I predict that when I increase the concentration of the hydrochloric acid the reaction will
take place quicker so more gas (CO2) will be produced in a shorter amount of time. I think
this will happen because at a higher temperature the ions have more kinetic energy so they
move through the solution faster so the ions will collide more often and more vigorously
meaning there is a greater chance they will react as reactions happen when ions collide. And I
predict that when I draw my graph showing the results, the line of best fit will go through
the origin because if the experiment is given no time for the reactions to take place then no
gas will be produced i.e. when the time is at zero (0) there will be no gas produced but as
time goes on more gas will be produced.
APPARATUS /MATERIALS
Thermometer
Beaker.
Measuring cylinder.
Electronic scales.
hydrochloric acid (0.5-2.5m)
30g of calcium carbonate (marble chips)
Timer
Clamp.
Stand.
Gas syringe
Bung
Calculator
Pipette
[Type text]

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JOAN NSIMBI
For safety I will wear safety goggles to protect my eyes from the
possibility of the acid splashing on my face. I will also wear a
protective lab coat to stop the acid splashing and burning my clothes
and skin since acid is highly corrosive and can cause serious injuries if gets in contact with
the skin.
PROCEDURE/ METHOD
Measure out 50cm³ of 1 molar Hydrochloric Acid and pour this
into a small beaker.…read more

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JOAN NSIMBI
MY TABLE OF RESULTS
THE VOLUME OF CARBON DIOXIDE (cm3) PRODUCED WITH 0.5M OF HCL.
Time(sec) Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Mean
cm3 cm3 cm3 cm3 cm3 cm3
20 15 16.5 14 14 10 14.8
40 17 16.5 17 11 17 16.8
60 20 21 15 20.5 20 20.4
80 21 22 22 22 17 21.8
100 30 30 30.5 25 31 30.4
120 32 33 33 34 19 33.…read more

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JOAN NSIMBI
THE VOLUME OF CARBONDIOXIDE PRODUCED (cm3) WITH 2.0 M OF HCL.
TIME(sec) TRIAL 1 TRIAL 2 TRIAL 3 TRIAL 4 TRIAL 5 MEAN cm3
cm3 cm3 cm3 cm3 cm3
20 16.5 18.5 16 16 11 16.7
40 19 18 18 13 19 18.5
60 23 23.5 40.5 22 22 22.6
80 22.5 25 23 24 18 23.6
100 32 31.5 32 26.5 33 32.1
120 34 35 34.5 35.5 20 34.7
THE VOLUME OF CARBONDIOXIDE (CM3) PRODUCED WITH 2.…read more

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JOAN NSIMBI
This makes it more reliable than a measuring cylinder. If I had used the burette my results
would be more reliable.
My readings of the amount of gas produced would have been easier to collect using a data
logo other than using the gas syringe.
MY FRIEND'S TABLE OF RESULTS
THE VOLUME OF CARBON DIOXIDE (CM3) PRODUCED WITH O.5M OF HCL.…read more

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JOAN NSIMBI
100 32 31.5 33 26.5 32.5 32.5
120 33 34.5 33 34 20 33.…read more

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JOAN NSIMBI
THE VOLUME OF CARBONDIOXIDE (CM3) PRODUCED WITH 2.0 M OF HCL.
TIME(sec) TRIAL 1 TRIAL 2 TRIAL 3 TRIAL 4 TRIAL 5 MEAN cm3
cm3 cm3 cm3 cm3 cm3
20 16.5 18.5 16 16 11 16.7
40 19 18 18 13 19 18.5
60 23 23.5 40.5 22 22 22.6
80 22.5 25 23 24 18 23.6
100 32 31.5 32 26.5 33 32.1
120 34 35 34.5 35.5 20 34.7
THE VOLUME OF CARBONDIOXIDE (CM3) PRODUCED WITH 2.…read more

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JOAN NSIMBI
When taking my results into consideration, I think my experimental results are not reliable
because the amount of gas produced is supposed to double as you increase the
concentration of hydrochloric acid. The possible cause of my results not being reliable is that
I had no time to allow the reaction to complete.…read more

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