1
124 = 0.0081 moles of CO2
0.0081 = 0.0020 moles of O2
4
= 0.0103 moles of gas produced for 1g of CuCO3.
0.0103 x 24000 = 247.2cm3
Equation 2
1g of CuCO3 will produce 194.4cm3 of gas.
0.0081 moles of Co2.
0.0081 x 24000 = 194.4cm3
Using this we can find out which equation is correct by the amount of gas produced.
Apparatus
Conical Flask
Rubber Tubing
Rubber Bung
Clamp Stand
Clamp
Gauze
Water Bowl
Bees Hive
Measuring Cylinder (500cm3)
Heat Proof Mat
Bunsen Burner
Copper Carbonate (At least 4g)
Stop Watch
Diagram
Variables and Fair Test
In this experiment I want to keep everything the same so I don’t get anomalous results. The Copper Carbonate will need to be heated so the gas given off will also be hot, because of this the gas will need to be left to cool before being recorded. When weighing the copper carbonate first zero the scales with the conical flask on them then put 1g of Copper Carbonate in the flask. If the first result is anomalous then you should discard it as a ‘practice run’. Between each experiment the conical flask will need to be cleaned well. Try and keep the equipment the same in each experiment as this may cause anomalous results. I have chosen to use a measuring cylinder over using a gas syringe because the gas syringe although accurate only holds 100cm3 of gas. The margin of error is smaller than using a gas syringe because the amounts of gas are so big, this means that using a less accurate measuring cylinder will not matter. Some of the CO2 will dissolve in the water but it is not enough to disrupt the results to much, BE AWARE the amount of gas in the cylinder will not be exactly the same as my prediction.
Method
- Get the required apparatus and set them up as in the diagram.
- Weigh out 1g of the Copper Carbonate as shown in the ‘Fair Test’ paragraph.
- Heat the Copper Carbonate using the Bunsen burner and collect the gas given off in the measuring cylinder.
- Leave the gas cool for five minutes.
- Record the amount of gas in the measuring cylinder.
- Repeat steps 2-5 four times, if the first result in anomalous then discard it.
- Get an average of the amount of gas from all reliable attempts.
-
If the average is nearest to 247.2cm3 then the first equation is correct. If it is about 194.4cm3 then the second equation is correct.
SAFTY: Always wear goggles when performing experiments in labs.
Bibliography
CHEMISTRY- Hunt, J A and Sykes, A
FOUNDATION CHEMISTRY- Raffan, John and Ratcliff, Brian
CHEM FACTSHEET- September 2000, Number 2
GROLIER MULTIMIDIA ENCYCLOPIDIA- 1996 CDROM
INFOPIDIA MULTIMIDIA ENCYCLOPIDIA- 1996 CDROM