Investigating the reaction between Bromine and Cyclohexane

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Chemistry titration coursework

Investigating the reaction between

Bromine and Cyclohexane

The outline of my experiment

By adding bromine to a mixture of Cyclohexane and water, and placing the mixture under a bright light and shaking from time to time, Hydrogen Bromide is formed. This reaction is shown below:

C6H12 + Br2                         C6H11Br + HBr

 

When the bromine has all reacted and the red colour has gone, the hydrogen bromide can be titrated with sodium hydroxide. This reaction is shown below:

 

HBr + NaOH                       NaBr + H2O  

From this titration I can then work out the HBr formed per mole of Bromine.

Results of my experiment

Class results.

Working out the mean averages

To work out the mean averages I used the following formula:

Sum of column / number of groups

My results- with raw data

Using the results

Bromine

I used a mass of 1.03grams of Bromine.

I arrived at this amount by weighing the volumetric flask without the bromine added then I weigh the flask with the bromine added. The different between which was 1.03 hence the mass of bromine must be 1.03to 2dp.

Moles

Mass of bromine used/ relative molecular mass of Br2= 1.03/(2x79.90)=0.00645to 3sf

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Sodium Hydroxide

I used 32.60cm3 of NaOH during the titration.

I arrived at this answer by recording an initial and final burette readings and then working out the difference, which was 32.60cm3.

Moles

Number of moles = concentration x volume (in dm3)= 0.200 x 0.03260= 0.00652 mol

The reaction

The reaction between the sodium hydroxide and hydrogen bromide is shown below:

 

  HBr + NaOH                        NaBr + H2O

Moles of Hydrogen Bromide produced in the reaction between Bromine and Cyclohexane

Number of moles of Bromine used ...

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