• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2

# In this experiment we hope to find the formula of a compound - a yellow compound formed when copper reacts directly with iodine vapour.

Extracts from this document...

Introduction

Experiment. In this experiment we hope to find the formula of a compound - a yellow compound formed when copper reacts directly with iodine vapour. Apparatus. Copper Strip, emery paper, dry filter paper, access to a balance, iodine crystals, boiling tube and a Bunsen burner. Method. We took a strip of copper and cleaned it with emery paper. Following this, we weighed the strip on a top pan balance. We placed the strip of copper into a boiling tube with the end bent around the lip of the boiling tube. ...read more.

Middle

A purple gas was emitted from the iodine crystals when heated and as the experiment continued, an obvious change in colour of the copper strip was apparent. We continued to heat the boiling tube until no purple gas was seen. Results. Initial Mass of copper strip 1.332g Mass of copper strip + copper iodide 1.608g Final mass of copper strip 1.191g Mass of copper that has reacted with the iodine: 0.141g Mass of iodine it reacted with: 0.276g No. of moles of copper atoms reacted (Ar Cu=63.5): 0.0022205 No. ...read more.

Conclusion

Another error may have been that we lost a substantial amount of the purple vapour while heating the test tube and this would affect the amount of copper iodide formed on the copper. Uncertainties, or experimental errors, would include the weighing of the masses. When weighing the masses of the copper strip, the copper iodide, etc. we used top-pan balances. Top-pan balances round off masses to a certain degree of accuracy and our balances read off at 2dp. The experimental error here is that there is a small space for error to occur in the rounding off process. This is called percentage error. Percentage error = error x 100 Reading Therefore : 0.005g x 100 = 0.04% 11.46g ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Classifying Materials section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related GCSE Classifying Materials essays

1. ## Investigation to Identify the Formula of Hydrated Copper Sulphate and in doing so Find ...

volume; faint green tinge evident during heating 9.309 Fine white powder formed; began to cluster - required breaking up with glass rod ? 0.002 2nd 9.309 Olive green tinge becomes more evident as heating continues 9.292 Powder appears slightly grey after heating ?

2. ## Identification of an unknown compound.

Finally, add aqueous ammonia until the brown precipitate dissolves. This solution is tollens reagent, add to this, 1cm3 unknown compound. If an aldehyde is the organic unknown compound, a 'silver mirror' will form on the test-tube. However if no silver deposits are observed then a ketone will be identified as the unknown chemical.

1. ## The role of mass customization and postponement in global logistics

Peripherals: Are labels, packaging and instruction manuals common to all markets? Starting from the perspective of global brands only, there can be only four different combinations of answers to these questions, as indicated in Table I, using illustrations from consumer markets.

2. ## Relationship between mass of MgO and its formula

5cm Mg O Mass 0.1g 0.06g RAM 24 16 Moles= mass RAM 0.1= 0.004167 24 0.14= 0.00375 16 0.004167 =1.11 0.00375 0.00375=1 0.00375 Ratio 1.11:1 7.5cm Mg O Mass 0.16g 0.04 RAM 24 16 Moles= mass RAM 0.16= 0.006667 24 0.04= 0.0025 16 0.006667=1 0.006667 0.0025=0.375 0.006667 Ratio 1:0.375 10.0cm

1. ## Finding the empirical formula of aluminium chloride.

More significantly, are the random errors that may have occurred. The many measurements that were taken involved considerable individual judgement, such as making sure the bottom of the surface meniscus was in line with the calibration mark, and judging when the end-point had been attained, which in this case was quite faint.

2. ## Chemistry Coursework. Aim: To find out if the thickness of plastic bags is ...

* The third measurement I will take will be that of the mass of one strip from each plastic bag. I will use a digital balance to do this as it is accurate to 0.01 of a gram.

1. ## An experiment to investigate the factors that determine the amount of energy released when ...

The alcohols available in the laboratory range from methanol containing one carbon atom, up to hexanol, containing 6 carbon atoms. By applying the formula for molecular mass, mentioned in the input variables, we get the masses of 32g for methanol and 102g for hexanol.

2. ## Our experiment consisted of two samples of water containing unknown substances, and our objective ...

Record the volume. 6. After about 2-3 minutes of heating, turn of the gas tap since the evaporating basin shouldn't contain any traces of liquid by now. 7. Set up the scales by plugging it into the socket. Make sure the reading displays '0.00g'.

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to