How would you electroplate an iron spoon with copper? Describe with diagram
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Open the Yenka Model 1.Add one iron electrode and one copper electrode to the bath.
Connect the iron electrode to the battery (negative end) and the copper electrode to the switch (positive end). This means that the iron electrode is the cathode and the copper electrode is the anode.Add the copper sulfate solution to the bath until the electrodes are just covered.Close the switch.
Open the reaction details of the bath by clicking on the "i" on the bath's toolbar. As time passes, watch the concentrations of the copper sulfate solution. What happens to the concentration of the copper ion solution?AnswerReload the model and repeat the experiment, but this time replace the copper electrode with a carbon electrode. In this case, what happens to the concentration of the copper ion solution?
(Note: if the electrodes are quite far apart, it may take several minutes to see any change. You may wish to move the electrodes closer together or speed up the simulation time using the slider in the menu at the top of the screen.)AnswerWhen the cathode is iron and the anode is copper, copper metal is oxidised at the anode and copper ions are reduced at the cathode. Write half-equations to describe these processes.AnswerExplain why it is advantageous to use an anode that is the same metal as the metal to be deposited on the cathode.AnswerNext, reload the model. This time, add a silver electrode as the anode and the iron spoonas the cathode. Connect the spoon to the circuit, but leave it sitting outside of the bath.Fill the bath with the silver nitrate solution, then close the switch.Finally, dip the spoon into the bath and allow electroplating to take place for about 30 seconds. What has happened?AnswerMetals can be arranged in order of decreasing reactivity. For example: Potassium > Sodium > Calcium > Magnesium > Zinc > Iron > Tin > Lead > Copper > Silver > Gold.
Explain why it might be advantageous to coat the iron spoon with silver.AnswerSummary
Connect the iron electrode to the battery (negative end) and the copper electrode to the switch (positive end). This means that the iron electrode is the cathode and the copper electrode is the anode.Add the copper sulfate solution to the bath until the electrodes are just covered.Close the switch.
Open the reaction details of the bath by clicking on the "i" on the bath's toolbar. As time passes, watch the concentrations of the copper sulfate solution. What happens to the concentration of the copper ion solution?AnswerReload the model and repeat the experiment, but this time replace the copper electrode with a carbon electrode. In this case, what happens to the concentration of the copper ion solution?
(Note: if the electrodes are quite far apart, it may take several minutes to see any change. You may wish to move the electrodes closer together or speed up the simulation time using the slider in the menu at the top of the screen.)AnswerWhen the cathode is iron and the anode is copper, copper metal is oxidised at the anode and copper ions are reduced at the cathode. Write half-equations to describe these processes.AnswerExplain why it is advantageous to use an anode that is the same metal as the metal to be deposited on the cathode.AnswerNext, reload the model. This time, add a silver electrode as the anode and the iron spoonas the cathode. Connect the spoon to the circuit, but leave it sitting outside of the bath.Fill the bath with the silver nitrate solution, then close the switch.Finally, dip the spoon into the bath and allow electroplating to take place for about 30 seconds. What has happened?AnswerMetals can be arranged in order of decreasing reactivity. For example: Potassium > Sodium > Calcium > Magnesium > Zinc > Iron > Tin > Lead > Copper > Silver > Gold.
Explain why it might be advantageous to coat the iron spoon with silver.AnswerSummary
The process of electrolysis is used to cover one metal with another for decorative or protective reasons. The object to be plated is made the negative electrode (cathode) in the electrolysis of a solution containing the ions of the plating metal. The positive electrode (anode) is usually made of the plating metal.
Suppose the plating metal is silver. The reaction on the metal being plated is:
Ag+(aq) + e− → Ag(s)
While the reaction at the anode is:
Ag(s) → Ag+(aq) + e−
Using an anode made of the plating metal has the advantage of replacing the ions of silver that have been converted to solid silver on the surface of the object.
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