• 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
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10
  11. 11
    11
  12. 12
    12

GCSE Chemistry - Electrolysis Coursework

Extracts from this document...

Introduction

��ࡱ�>�� KM����J�������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������5@ ��0�.bjbj�2�2 (b�X�X!$�������������������8� ����v��������tvvvvvv$kR���������������BBB�����tB�tBBT��T�� ���QO����dTt�0�T� � T������� �T ��B�������2GCSE Chemistry - Electrolysis Coursework AIMS It is known that by passing a constant electric current through an aqueous copper sulphate solution that the passage of ions through this solution results in copper atoms being dissolved into the solution from the anode while positive copper ions (cations) being discharged at the cathode. Normally anions are discharged at the anode. The experiment carried out aimed to monitor the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. It was considered that the following factors could affect the deposition of Copper metal on the cathode. 1. Time 2. Current 3. Temperature 4. Molarity/Concentration of Solution 5. Quantity of Solution 6. Size of Electrodes 7. Distance between the electrodes 8. The surface of the electrodes The time was chosen because it is an easy quantity to measure and record, whilst at the same time maintaining the other variables at a constant level. The other factors could be observed in later experiments, should time allow. PREDICTIONS It is possible to predict that the relationship will be directly proportional between the time the current flows and the mass of Copper deposited on the Cathode (negative electrode). ...read more.

Middle

The electrodes were weighed, their masses recorded and placed into the beaker containing Copper Sulphate solution. The electrodes were connected to a cell and ammeter. A steady current flowed (0.2 Amps) and the experiment was stopped at definite times (i.e. 5,10,15,20,25 minutes). At these times the current was switched off and both electrodes were removed from the solution. They were then washed by dipping in distilled water, and dried by dipping into propanone (a highly volatile liquid which readily evaporates) and placed near an electric heater. Once clean and dry both electrodes were both carefully weighed and their subsequent masses recorded. RESULTS ANODE (+) TIME (MINUTES) ORIGINAL MASS OF ANODE (grams) FINAL MASS OF ANODE (grams) CHANGE IN MASS AT ANODE (grams) 5 12.491g 12.468g -0.023g 10 11.834g 11.792g -0.042g 15 12.528g 12.459g -0.069g 20 12.444g 12.365g -0.080g 25 11.098g 11.002g -0.096g CATHODE (-) TIME (MINUTES) ORIGINAL MASS OF CATHODE (grams) FINAL MASS OF CATHODE (grams) CHANGE IN MASS AT CATHODE (grams) 5 11.824g 11.848g +0.024g 10 12.456g 12.485g +0.039g 15 12.942g 13.011g +0.069g 20 12.967g 13.050g +0.082g 25 13.872g 13.983g +0.111g AVERAGE TIME (MINUTES) AVERAGE CHANGE IN MASS (grams) 5 0.0235g 10 0.0405g 15 0.0690g 20 0.0810g 25 0.104g THEORETICAL RESULTS TIME (MINUTES) THEORETICAL CHANGE IN MASS (grams) 5 0.0199g 10 0.0398g 15 0.0597g 20 0.0796g 25 0.0995g CONCLUSION The results obtained support the prediction that the longer the current is left to flow, the more Copper metal is deposited on the cathode. ...read more.

Conclusion

The UK's Coursework Database - http://www.coursework.info/ This document was downloaded from Coursework.Info - The UK's Coursework Database - http://www.coursework.info/ This document was downloaded from Coursework.Info - The UK's Coursework Database - http://www.coursework.info/ �Z ,!,�,�,--s-t-�-�-W.X.�.�.�.�.�������������ho9�ho9�OJQJho9�ho9�CJOJQJ%ho9�ho9�OJQJfHq� ����)ho9�ho9�CJOJQJfHq� ����ho9�hgT�ho9�ho9�mHsH hgT�ho9�)*0123� � � � � � � � � � � � � � � � 0 1 2 �����������������������������gdgT�!,�.��2 3 O P Q R l m n o � � � � � � � � � � � � � � %&'(+,�����������������������������gdgT�,-._`ab��������&'()����?@ABTUV�����������������������������gdgT�VWghij~������FGHI���� GHIJ�����������������������������gdgT�J��������������BCDEabcd~�����������������������������gdgT�~��������������9:;<VWYZ�������������������������������gdgT����������������/012ghij��������������������������������gdgT��������������� ?@ABabcd��������������������������������gdgT��������������2345<=>?qrstwxyz������������������������������gdgT�����������'(=>?@HIjkmnpqz{���������������������������������gdgT������������������������������������������������������������gdgT���"#%&'(4567FGij�����������������������������������gdgT�����������������������������������������������������gdgT�"#,-67@ACDGHQR[\efhijkstuv�������������������������������gdgT������������������������������������������������������������gdgT���������%&JKMNPQZ[]^abklno�����������������������������gdgT�ors|}������������������ � � � � � :!�����������������������������gdgT�:!;!<!=!y!z!{!|!B"C"D"E"�"�"�"�"�"�"�"�"�"�"9#:#;#<#m#n#o#p#�����������������������������gdgT�p#�#�#�#�#�#$$$4$5$6$7$�$�$�$%x%y%z%{%�%�%�%�%�%�%�%�%�%�����������������������������gdgT��%�%�%�%�%�%�%�%�%�%�%�%�%�%�%�%((((+ + + +,,,,,,�����������������������������gdgT�,,,,, ,!,�,�,�,�,----t-u-v-w-�-�-�-�-X.Y.Z.[.��������������������������$a$gdo9�$a$gdo9�gdgT�[.�.�.�.�.�.�.������gdgT�$a$gdo9�&1�h:pgT���/ ��=!�'"�'#��$��%��D@�D NormalCJ_H aJmH nHsH tHDA@�D Default Paragraph FontRi�R Table Normal�4� l4�a� (k�(No ListDZ@�D gT� Plain TextCJOJQJ^JaJ4@4 o9�Header ���!4 @4 o9�Footer ���!`�o"` o9�watermark header$a$CJOJQJfHq� ����N�o2N o9�watermark footer$a$ CJOJQJ�&b����r�V�:���.2 ,VJ~���������o:!p#�%,[.�. !"#$%&'()*+,-./0�.� Z $!$�$�$%%u%w%�%�%Y&[&�&�&� � $�& $�&��alex�gT�o9��@!$`���&P@��Unknown������������G��z ��Times New Roman5V��Symbol3&� �z ��Arial7&� � �VerdanaG5�� �����h�MS Mincho-�3� fg?5� �z ��Courier New"1���hQ �FQ �FQ �F���/���/$�������4�%�%3�� H�?������������������gT���(GCSE Chemistry - Electrolysis CourseworkTCoursework.Info Coursework - http://www.coursework.info/ - Redistribution ProhibitedTCoursework.Info Coursework - http://www.coursework.info/ - Redistribution Prohibitedalexalex�� ��Oh��+'��0����4D�� 8 D P \hpx��)GCSE Chemistry - Electrolysis Coursework WoUCoursework.Info Coursework - http://www.coursework.info/ - Redistribution ProhibitedualexewoUCoursework.Info Coursework - http://www.coursework.info/ - Redistribution Prohibitedu>Downloaded from Coursework.Info - http://www.coursework.info/is Normal.dotfalexl.d2exMicrosoft Word 10.0@@f�3O��@f�3O��@f�3O������ ��Õ.��+,��D��Õ.��+,���D���H����� ���� � %�UCoursework.Info Coursework - http://www.coursework.info/ - Redistribution ProhibitedtryUCoursework.Info Coursework - http://www.coursework.info/ - Redistribution ProhibitedtryUCoursework.Info Coursework - http://www.coursework.info/ - Redistribution Prohibitedtryf&/��%A )GCSE Chemistry - Electrolysis Coursework Titled@���+K_PID_LINKBASE CopyrightDownloaded FromCan RedistributeOwner�A4http://www.coursework.comcoursework.comehttp://www.coursework.comCoNo, do not redistributecoursework.com/ !"#$%&'()*+,-./01����3456789����;<=>?@A����CDEFGHI��������L����������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������Root Entry�������� �F�QO��N�1Table��������2WordDocument��������(bSummaryInformation(����:DocumentSummaryInformation8������������BCompObj������������j������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������������ ���� �FMicrosoft Word Document MSWordDocWord.Document.8�9�q ...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 Changing Materials - The Earth and its Atmosphere 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

See related essaysSee related essays

Related GCSE Changing Materials - The Earth and its Atmosphere essays

  1. GCSE Chemistry - Electrolysis Coursework

    Ø Moles of Electrons or Faradays = Charge (C) / 96500 Ø Moles of Copper = Moles of electrons or Faradays / ratio=2 Ø Mass = moles x RAM If the Current is 0.2A and the time taken 5 minutes Ø Charge = 0.2 x (5x60) Ø Faradays = 60/96500 Ø Moles of Copper = 0.0006217/2 Ø Mass =

  2. The Electrolysis Of Copper (ii) Sulphate Solution Using Copper Electrodes

    1 2 3 4 5 Temperature increase (0C) 6.00 6.75 8.00 9.00 10.25 Mass increase (g) - 0.08 - - 0.20 The mass increases were reasonable even after two minutes. However the temperature increases were much too large even after two minutes so only those under two minutes were suitable

  1. Investigation to show how the amount of electric current affects the amount of copper ...

    2.51 0.15 1.0 1.57 1.39 -0.18 2.51 2.70 0.19 1.0 2.34 2.15 -0.19 1.97 2.16 0.19 1.0 2.15 1.97 -0.18 2.16 2.38 0.20 1.0 1.97 1.77 -0.20 2.36 2.58 0.22 (the minus sign indicates a decrease in mass) Here are the averages of my experiment: Current (amps) Anode Before (grams)

  2. Investigation into Electrolysis

    As we were using such small amounts of substance, more emphasis should be placed on the observations rather than the measurements we attempted as their accuracy is unknown. The quantitative results confirm that the metal was electroplated in part A of stages 1 and 2.

  1. Factors affecting mass of copper transferred in Electrolysis of aqueous copper sulphate

    Diagram Apparatus list * 200cm� copper sulphate * wires * variable resistor * ammeter * power pack * 2 copper electrodes * 2 crocodile clips * stopwatch * scales * sandpaper Safety Precautions It is important to conduct the experiment in a safe way so overalls should be worn in

  2. Investigate the factors that affect the mass of Copper deposited on the Copper Cathode ...

    sulphate solution and this is predicted because it's atoms give up electrons to form ions in the solution Cu atom - 2e ==> Cu ion I also predict that the opposite occurs at the cathode, the copper ions pick up electrons and become copper atoms Cu + 2e ==> Cu

  1. Investigating the factors that affect the amount of copper deposited during the electrolysis of ...

    These are: a) the size of current passing through the cell b) the time for which the current passes through the cell c) the concentration of the copper sulphate solution d) the distance the electrodes are apart. If we vary one or more of the above factors, the amount of copper deposited on the cathode will change.

  2. The experiment carried out aimed to monitor the quantity of Copper (Cu) metal deposited ...

    � Moles of Electrons or Faradays = Charge (C) / 96500 � Moles of Copper = Moles of electrons or Faradays / ratio=2 � Mass = moles x RAM If the Current is 0.2A and the time taken 5 minutes � Charge = 0.2 x (5x60) � Faradays = 60/96500 � Moles of Copper = 0.0006217/2 � Mass =

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