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Formal Report on Iodine Clock Reaction. Please use this only as a guide. No to plagiarism :D Thanks. Hoping this will be able to help you in your studies.
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Formal Report on Iodine Clock Reaction. Please use this only as a guide. No to plagiarism :D Thanks. Hoping this will be able to help you in your studies.Descripción completa
octave
2/13/2013
REDEEMER LUTHERAN
EXPERIMENT 3- OBSERVING A CHEMICAL REACTION
COLLEGE
Teacher: Ms. Andress | Winston Boon
Experiment 3- Observing a Chemical Reaction Aim: To learn how qualitative and quantitative observations of a chemical reaction are used to formulate a hypothesis.
Hypothesis: In this experiment, we will be able to make assured qualitative and quantitative observations. Qualitative data will be when the aluminium foil is placed in the copper chloride. Quantitative data will be the initial and final temperature of the water.
Method: As on page 33 in the Chemistry Lab Manual
Materials: As on page 26 in the Chemistry Lab Manual
Risk Assessment: As on page 26 in the Chemistry Lab Manual
Do not come in contact with the copper chloride dihydrate through the air (no inhaling), drinking water and from foods as it may cause nausea, vomiting, diarrhoea, liver damage, kidney damage, may also result to death.
Using your hand as a fan to pick up the scent of the copper chloride will decrease your chances of taking a risk.
Copper Chloride Dihydrate
1|Page
Data Table(s): Data Table 1: Observations System
Observations
Dry Copper (II) Chloride Dihydrate
Turquoise in colour, soft, powdery look (using the rod to stir the dry copper), strong smell
Copper (II) Chloride in water
Soluble, Bubbling colour turned darker, foam was formed on the surface, no change in temperature
Stirred Copper (II) Chloride in water
The liquid turned blue in colour, bits of powder at the bottom of the beaker dissolved
Copper (II) Chloride Solution + Aluminium
Gas was produced, foil was decomposing into a brown dark red-like colour
Initial Temperature
24
o
Final Temperature
37
o
Data Table 2: Temperatures/min Time
Temperature [ 24o (Initial Temperature)]
1
37
o
2
47
o
3
46.5
4
45
o
5
44
o
6
41
o
7
40
o
8
39
o
9
37
o
10
37
2|Page
o
o
Analysis- Questions: 1. 2.
(Crossed out interpretations are shown above) A) Observations of the dry crystals
Turquoise in colour
Powdery look
Soft (when using the rod to move crystals around)
Strong smell
B) Observations of the wet crystals before stirring
Becomes soluble instantaneously without the use of stirring
Bubbling
Colour turned darker
No change in temperature
C) Observations of the solution before addition of the aluminium
A change in colour from green to blue
Some bits of powder on the bottom of the beaker dissolved
D) Observations of the reaction that occurs when the aluminium is added to the solution o
Initial Temperature- 24 degrees Celsius (24 C)
Bubbles were formed
Gas coming out from the beaker
Colour change; turned into a dark grey-like liquid
Red-like structure on the outside of the piece of aluminium which turned into a ball immediately after dropping into beaker o
Highest Temperature- peaked at 46.5 C
Aluminium ball completely changes into a red-like solid material
Final Temperature- finished at 37 C
Formula:
o
-
2Al(s) + 3CuCl2(aq) --> 3Cu(s) + 2AlCl3(aq)
aluminum ion in solution may be coordinated with four chloride ions: [AlCl4]-
-
Copper (II) ions will decompound to produce an excess of hydrogen ions, making the copper (II) chloride solution a little acidic.
3|Page
-
Aluminum metal is always enclosed in a thin, but protective coating of aluminum oxide, Al2O3. The chloride ion supports to disperse the aluminum from the oxygen so that the aluminum can react with the copper ions (and also the water molecules).
-
Cu2+ + HOH --> CuOH- + H+
Al2O3 + 4Cl- + H2O + 2H+ --> 2[Al(OH)2Cl2]-
The reaction is also maintained by the hydrogen gas
2Al + 6H+ --> 2Al3+ + 3H2
3.
The observations and interpretations collected and recorded are most likely to not match our classmates’ observations as each group may have attempted and accomplished the experiment
differently to others e.g. some groups may have stirred gradually after each minute, some may have not stirred at all and collected the initial and final temperature. Our group however collected the temperature every minute up to ten minutes. Thus the observations collected will not be expected to match other grou ps’ observations.
Conclusion: In conclusion, we made qualitative and quantitative observations thus learned how qualitative and quantitative observations of a chemical reaction are used to formulate a hypothesis. The observations and interpretations collected and recorded were conceivably recognisable of how qualitative and quantitative observations are used to form ulate hypothesises.
Error Analysis: Some improvements can be made in this experiment such as stirring the mixture from time to time every one minute without missing a single minute, counting the time segments more accurately and recording the temperature at least 2-3 seconds before one minute to wait until the temperature has started rising.
