• 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
13. 13
13
14. 14
14
15. 15
15
16. 16
16
17. 17
17
18. 18
18
19. 19
19

# Investigating how the amount of copper affects the mass of the cathode

Extracts from this document...

Introduction

INTRODUCTION: In this experiment I will be investigating how the amount of copper affects the mass of the cathode. I will do this experiment twice so that I have an average of my results so that they are accurate. I have already done my preliminary work and from it, I have noticed that I will have to make some changes with the method of my experiment. AIM: In this experiment, I intend to find out how much copper in the solution affects the mass of the cathode. I will be observing to see what is happening and exactly how much copper is being deposited on the cathode. Out of the four variables that are listed below, I will be concentrating on the time the electrodes are left in the solution and the size of current that will be applied in this experiment. VARIABLES: There are four variables, which affect this investigation. The first variable is the size of the current applied in the solution. As the current raises so does amount of electrons that are produced on the cathode. This means the anode loses its positively charged ions, which the cathode gains, which means more positive ions, will combine with the electrons on the cathode to produce copper. The second variable that affects the experiment is the amount of time the experiment is carried out for. The greater the time the electrodes are left in the solution, the more time there is for the copper to be gathered at the anode. The third variable that affects the experiment is the temperature of the copper II sulphate solution. As the temperature of the solution increases, more of the ions gain kinetic energy and begin to move faster. This enables the positive and negative charged ions to collide faster with the electrodes. As more of the positive and negative ions collide, there is a greater chance for the pure copper to be formed at the cathode. ...read more.

Middle

All these changes helped me to gain more accurate results than previously. RESULTS: Here are my results for both experiments. TIME (MINS) CURRENT (AMPS) STARTING MASS OF ELCTRODES (g) MASS OF ANODE (g) (AFTER 10 MINUTES) MASS OF CATHODE (g) (AFTER 10 MINUTES) CHANGE OF WEIGHT AFTER 10 MINUTES (g) 10 0.5 ANODE = 1.1 CATHODE =1.0 1.0 1.1 ANODE = -0.1 CATHODE = +0.1 20 0.6 ANODE = 1.0 CATHODE =1.1 0.9 1.2 ANODE = -0.1 CATHODE = +0.1 30 0.7 ANODE = 0.9 CATHODE= 1.2 0.7 1.4 ANODE = -0.2 CATHODE = +0.2 40 0.8 ANODE=0.7 CATHODE =1.4 0.5 1.6 ANODE = -0.2 CATHODE = +0.2 50 0.9 ANODE = 0.5 CATHODE = 1.6 0.2 1.8 ANODE = -0.3 CATHODE =+0.2 TIME (MINS) CURRENT (AMPS) STARTING MASS OF ELECTRODES (g) MASS OF ANODE (g) (AFTER 10 MINUTES) MASS OF CATHODE (g) (AFTER 10 MINUTES) CHANGE OF WEIGHT AFTER 10 MINUTES (g) 10 0.5 ANODE = 0.9 CATHODE =0.9 0.8 1.0 ANODE =-0.1 CATHODE = +0.1 20 0.6 ANODE =0.8 CATHODE =1.0 0.6 1.2 ANODE = -0.2 CATHODE = +0.2 30 0.7 ANODE =0.6 CATHODE=1.2 0.4 1.4 ANODE = -0.2 CATHODE = +0.2 40 0.8 ANODE =0.4 CATHODE =1.4 0.3 1.5 ANODE = -0.1 CATHODE = +0.1 50 0.9 ANODE =0.3 CATHODE =1.5 0.1 1.7 ANODE= -0.2 CATHODE =+0.2 TIME (MINS) CURRENT (AMPS) CHANGE OF MASS AFTER 10 MINUTES EXPERIMENT 1 CHANGE OF MASS AFTER 10 MINUTES EXPERIMENT 2 AVERAGE OF EXPERIMENT 1 AND EXPERIMENT 2. (g) ANODE CATHODE ANODE CATHODE ANODE CATHODE 10 0.5 -0.1g +0.1g -0.1g +0.1g -0.1g +0.1g 20 0.6 -0.1g +0.1g -0.2g +0.2g -0.15g +0.15g 30 0.7 -0.2g +0.2g -0.2g +0.2g -0.2g +0.2g 40 0.8 -0.2g +0.2g -0.1g +0.1g -0.15g +0.15g 50 0.9 -0.3g +0.2g -0.2g +0.2g -0.25g +0.2g To find out the average mass of the cathode : Experiment 1 + Experiment 2 2 GRAPHS: The graph below shows the average results of both experiments. ...read more.

Conclusion

If I have to carry this investigation out once again, I would make sure that I make the following improvements. I would use a device to make sure that the temperature of the solution is constant all the way through because previously I noticed that the temperature was not constant and increased as more current was applied, which was not a fair test. I would also use bigger electrodes so that I can continue this experiment on for a longer period allowing me to gain a larger number of results as well as results that are more accurate. I would also use a top pan balance that was maybe up to three decimal places instead of one decimal place. This is because every time that I weighed the electrodes, I sometimes noticed that the mass had not changed much as it should have or sometimes the mass did not change at all. If there were a three decimal place balance, I would gain more accurate results, graphs as well as for a more precise conclusion. I would also increase the time of the electrodes that are left in the solution so I could investigate further. I would also investigate the other our variables to see if there is any difference in the results. Overall, I thought that my experiment went fairly well. I tried to keep to the safety aspects as well as trying to lead a fair test. The majority of the experiment was fair and I gained reliable results that proved the majority of my hypothesis. Also my hypothesis and prediction was correct and did prove the majority of the results gained except for a few which I have accounted for already. From this experiment, I learnt about electrolysis in more depth as well as learning more about Michael Faraday and his two laws of electrolysis (stated above in the hypothesis). I have also learnt were I have to improve in carrying out this experiment as a fair test which I have already explained earlier on. 1 ...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

# Related GCSE Changing Materials - The Earth and its Atmosphere essays

1. ## To find out how current affects the rate of electrolysis

3 star(s)

If the copper is extracted the solution would turn clear. I predict that the hydroxide would form on the anode. This is because the negative ions in the solution are the sulphate ion SO42-, and the hydroxide ion OH-. These will migrate to the positive anode.

2. ## The aim of this experiment is to determine the order of the reactivity series ...

Manganese is about as reactive as Magnesium. I think that Manganese lies just below Magnesium in the reactivity series, and above Aluminium. Evaluation I think that the Iron Carbonate being the metal which thermally decomposed the fastest was an anomalous result.

1. ## How does concentration affect the rate of electrolysis of Copper Sulphate solution?

0.95 23 23.5 1 0 0.82 23 23 Average: Table 5 Concentration (ml) Current (MA) Temperature (�C) mol/dm� water Initial End 0.5 0.5 0.69 22.8 23.8 0.6 0.4 0.75 22.7 23.3 0.7 0.3 0.85 22.7 23.7 0.8 0.2 0.85 23 24 0.9 0.1 1.00 23.5 24.3 1 0 1.02 23 23.5 Graph of Average results with sloping line: Fig.

2. ## To determine the value of Faraday constant (quantity of electricity per mole) by using ...

That's why the gain in weight of the cathode was not taken in account when calculating the Faraday Constant. The loss in weight in anode should always be larger than the gain in weight of the cathode. On the other hand, during electrolysis, it couldn't be confirmed that the copper

1. ## Electrolysis: How Does Current Affect The

The ions and electrons combine together to form copper metal. If more ions are present then the speed will increase and so will the mass of copper collected. Evaluation: I used a very easy method to follow, because there was not much to change.

2. ## An experiment to show how electroplating using copper electrodes.

Next averages are found. 9. These should be put into a table. PRELIMINARY ANALYSIS From my previous found out, stated out in a table it shows what figures should be used for the real experiment The experiment was timed for a fixed time interval of five minutes.

1. ## The Electrolysis Of Copper Sulphate Solution Using Copper Electrodes

Copper electrodes are not inert, instead of incoming anions being discharged, the copper goes into solution: Cu(s) > Cu" (aq) + 2e- The reaction occurring at the anode during the electrolysis of a copper salt is the reverse of the cathode reaction.

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

sulphate solution, the more time there will be for cu 2+ ions to be deposited. * Current If the current is larger, there will be more electrons flowing around the circuit and more copper will be deposited. * Temperature The greater the temperature the more copper deposited at the cathode

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