• 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
3. 3
3

# Finding the Empirical Formula of a Compound

Extracts from this document...

Introduction

Lab - Finding the Empirical Formula Aim: To investigate a compound and determine its empirical formula. In this assessment, we find x in the formula: CuS04.xH20 by removing the water of crystallization from hydrated copper(II) sulphate by heating it, and then using the empirical formula method of calculation to work out the formula. Apparatus: Crucible, Bunsen Burner, Tripod, Pipe clay triangle, and a sample of the compound (I took CuSO4 . xH2O, where x is an unknown constant we need to find to determine the empirical formula. Method: 1. The apparatus was set up as shown in the diagram below. 2. ...read more.

Middle

Trial Number Original Mass of compound � 0.01 g Final Mass � 0.01 g Mass of Copper Sulphate � 0.01 g Mass of Water lost � 0.01 g 1 2.00 1.24 1.24 0.76 2 0.46 0.26 0.26 0.20 The data from Trial 1 was then used to calculate the empirical formula CuSO4 H2O Calculations for CuSO4 Calculations for H2O Masses of Compounds 1.24 0.76 Molar Mass 160 18 64 + 32 + (4 x 16) 2 x 1 + 16 No. of Moles 0.00775 0.042222 1.24 / 160 0.76 / 18 Ratio of Moles 1 : 5.448029 CuSO4 : H2O :: 1 : (0.04222 / 0.00775) ...read more.

Conclusion

7H2O Conclusion: From the results obtained, it seems like the empirical formula of the compound is CuSO4 . 5H2O or CuSO4 . 7H2O . However, the theoretical result we should have obtained is CuSO4 . 5H2O . Hence, there have been some large errors in the second trial. The results wasn't taken as an average of the two results obtained, as the second results was erroneous due to mistakes made during the experiment. Evaluation: Evidently, the first experiment was quite accurate, as the theoretically expected results were achieved. However, the second experiment was grossly inconsistent, which indicates that there have been some random errors. The second set of results is faultier, but this is because some of the Copper Sulphate fell out of the crucible while measuring its mass. ...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. ## Determine the formula of the hydrate in hydrated copper (II) sulfate empirically, i.e. to ...

See: CuSO4 xH2O 1.267g ? 0.004g 0.767g ? 0.008g Using the formula: n = m/M, where n = moles, m = mass of sample, and M = molar mass of compound n(CuSO4) = 1.267g/[63.55 g.mol-1 + 32.06 g.mol-1 + 4(16.00)

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

Results: Fig. 1 A Table to Show Key Masses COMPONENTS MASS (g) |ERROR|(g) Crucible 8.024 ? 0.002 Crucible and CuSO4 � xH2O 10.058 ? 0.002 NOTE: Systematic error associated with electronic balance is consistently ? 0.002 g Initial observations of hydrated copper (II)

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

Although from the calculations I made using the empirical formula do not show a perfect relationship (in this case composition) which would ideally be 1:1, my results are not far off it. For example take the results I obtained from 5cm of magnesium, using the empirical formula I was able

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

Now the nozzle can let more oxygen in, the flame will be hotter and a different colour, dark blue. The evaporating process can take place now, since the flame can give out more heat. Because the flame is so hot, it would be very dangerous to put your finger through it.

1. ## Identification of an unknown compound.

If the unknown chemical is either an aldehyde or a ketone, an orange/yellow precipitate will form. If a positive result occurs and an orange/yellow precipitate forms, proceed to test 3 (silver-mirror test), to distinguish between aldehydes and ketones. If no orange/yellow precipitate forms skip test 3 and continue to test 4.

2. ## Determination of the formula of hydrated iron sulphate

+16 Moles of H2O = 0.0362 correct to 3 significant figures To calculate the formula of FeSO4. xH2O the smallest number of the two values for the moles of FeSO4 and H2O needs to be made to 1 and the ratio then calculated.

1. ## Determination of the formula of Hydrated Iron (II) Sulphate Crystals

Mass of weighting boat and FeSO4: 4.85g * Mass of FeSO4 = Mass of weighting boat and FeSO4 - Mass of weight boat o = 4.85g - 1.87g = 2.98g * Moles of KMnO4 = concentration*volume * Concentration: 0.0100 moldm-3* * Volume: 18.85 cm2/1000 = 0.01885dm3 * Moles = 0.0100

2. ## An experiment to find the empirical formula when copper reacts with iodine

This means that for all the weights given by the scales, the actual weight is � 0.005 (g) of the value shown. In order to show what the precision error of different measurements means, they are normally expressed as a percentage using the following formula.

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