The Role of the Cathode in an Electrolytic Cell

Oct 13, 2025 by talynt.org 121 views

In an electrolytic cell, the cathode is the electrode where reduction occurs, and it is the site where the reduction reaction takes place. The cathode is typically the negatively charged electrode, and it is where the ions from the electrolyte are reduced to form a solid product. In the context of a nickel and copper electrolytic cell, we need to determine which of the given options would be the cathode.

The Role of the Cathode in an Electrolytic Cell

The cathode plays a crucial role in an electrolytic cell, as it is where the reduction reaction occurs. The reduction reaction involves the gain of electrons by the ions in the electrolyte, resulting in the formation of a solid product. The cathode is typically made of a material that is capable of conducting electricity, such as a metal.

The Cathode in a Nickel and Copper Electrolytic Cell

In a nickel and copper electrolytic cell, the cathode would be the electrode where the reduction reaction occurs. The reduction reaction would involve the reduction of the ions in the electrolyte to form a solid product. The options given are:

A. $$Ni^{2+}$$: This option represents the nickel ion, which is a cation. In an electrolytic cell, the cathode is typically the site where reduction occurs, and cations are reduced to form a solid product.
B. $$Cu^{2+}$$: This option represents the copper ion, which is also a cation. Like the nickel ion, the copper ion would be reduced to form a solid product at the cathode.
C. $$Ni(s)$$: This option represents solid nickel, which is a metal. In an electrolytic cell, the anode is typically the site where oxidation occurs, and metals are oxidized to form ions.
D. $$Cu(s)$$: This option represents solid copper, which is also a metal. Like solid nickel, solid copper would be oxidized at the anode, not reduced at the cathode.

Conclusion

Based on the understanding of the cathode in an electrolytic cell, the correct answer is A. $$Ni^{2+}$$ or B. $$Cu^{2+}$$. Both of these options represent cations that would be reduced to form a solid product at the cathode in a nickel and copper electrolytic cell.

In an electrolytic cell, the anode is the electrode where oxidation occurs, and it is the site where the oxidation reaction takes place. The anode is typically the positively charged electrode, and it is where the solid product is oxidized to form ions. In the context of a nickel and copper electrolytic cell, we need to determine which of the given options would be the anode.

The Role of the Anode in an Electrolytic Cell

The anode plays a crucial role in an electrolytic cell, as it is where the oxidation reaction occurs. The oxidation reaction involves the loss of electrons by the solid product, resulting in the formation of ions. The anode is typically made of a material that is capable of conducting electricity, such as a metal.

The Anode in a Nickel and Copper Electrolytic Cell

In a nickel and copper electrolytic cell, the anode would be the electrode where the oxidation reaction occurs. The oxidation reaction would involve the oxidation of the solid product to form ions. The options given are:

A. $$Ni^{2+}$$: This option represents the nickel ion, which is a cation. In an electrolytic cell, the anode is typically the site where oxidation occurs, and cations are formed from the oxidation of metals.
B. $$Cu^{2+}$$: This option represents the copper ion, which is also a cation. Like the nickel ion, the copper ion would be formed from the oxidation of a metal at the anode.
C. $$Ni(s)$$: This option represents solid nickel, which is a metal. In an electrolytic cell, the anode is typically the site where oxidation occurs, and metals are oxidized to form ions.
D. $$Cu(s)$$: This option represents solid copper, which is also a metal. Like solid nickel, solid copper would be oxidized at the anode, not reduced at the cathode.

Conclusion

Based on the understanding of the anode in an electrolytic cell, the correct answer is C. $$Ni(s)$$ or D. $$Cu(s)$$. Both of these options represent metals that would be oxidized to form ions at the anode in a nickel and copper electrolytic cell.

In an electrolytic cell, the cathode and anode are two electrodes that are connected by an external power source. The cathode is the site where reduction occurs, and the anode is the site where oxidation occurs. The relationship between the cathode and anode is crucial in understanding the operation of an electrolytic cell.

The Cathode and Anode in a Nickel and Copper Electrolytic Cell

In a nickel and copper electrolytic cell, the cathode and anode are connected by an external power source. The cathode is the site where reduction occurs, and the anode is the site where oxidation occurs. The options given are:

A. $$Ni^{2+}$$ and $$Ni(s)$$: This option represents the nickel ion and solid nickel, respectively. In an electrolytic cell, the nickel ion would be reduced to form solid nickel at the cathode, and solid nickel would be oxidized to form nickel ions at the anode.
B. $$Cu^{2+}$$ and $$Cu(s)$$: This option represents the copper ion and solid copper, respectively. Like the nickel ion and solid nickel, the copper ion would be reduced to form solid copper at the cathode, and solid copper would be oxidized to form copper ions at the anode.
C. $$Ni^{2+}$$ and $$Cu(s)$$: This option represents the nickel ion and solid copper, respectively. In an electrolytic cell, the nickel ion would be reduced to form solid nickel at the cathode, and solid copper would be oxidized to form copper ions at the anode.
D. $$Cu^{2+}$$ and $$Ni(s)$$: This option represents the copper ion and solid nickel, respectively. Like the nickel ion and solid copper, the copper ion would be reduced to form solid copper at the cathode, and solid nickel would be oxidized to form nickel ions at the anode.

Conclusion

Based on the understanding of the cathode and anode in an electrolytic cell, the correct answer is A. $$Ni^{2+}$$ and $$Ni(s)$$ or B. $$Cu^{2+}$$ and $$Cu(s)$$. Both of these options represent the relationship between the cathode and anode in a nickel and copper electrolytic cell.

Conclusion

In conclusion, the cathode in a nickel and copper electrolytic cell would be the electrode where reduction occurs, and it is the site where the reduction reaction takes place. The cathode is typically the negatively charged electrode, and it is where the ions from the electrolyte are reduced to form a solid product. The correct answer is A. $$Ni^{2+}$$ or B. $$Cu^{2+}$$.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Brown, T. E., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, P. (2012). Chemistry: The Central Science (13th ed.). Pearson Education.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Frequently Asked Questions (FAQs) About the Cathode in a Nickel and Copper Electrolytic Cell =============================================================================================

Q: What is the cathode in an electrolytic cell?

A: The cathode is the electrode where reduction occurs, and it is the site where the reduction reaction takes place. The cathode is typically the negatively charged electrode, and it is where the ions from the electrolyte are reduced to form a solid product.

Q: What is the role of the cathode in an electrolytic cell?

A: The cathode plays a crucial role in an electrolytic cell, as it is where the reduction reaction occurs. The reduction reaction involves the gain of electrons by the ions in the electrolyte, resulting in the formation of a solid product.

Q: What is the difference between the cathode and anode in an electrolytic cell?

A: The cathode and anode are two electrodes that are connected by an external power source. The cathode is the site where reduction occurs, and the anode is the site where oxidation occurs.

Q: What would be the cathode in a nickel and copper electrolytic cell?

A: The cathode in a nickel and copper electrolytic cell would be the electrode where reduction occurs, and it is the site where the reduction reaction takes place. The correct answer is A. $$Ni^{2+}$$ or B. $$Cu^{2+}$$.

Q: What would be the anode in a nickel and copper electrolytic cell?

A: The anode in a nickel and copper electrolytic cell would be the electrode where oxidation occurs, and it is the site where the oxidation reaction takes place. The correct answer is C. $$Ni(s)$$ or D. $$Cu(s)$$.

Q: What is the relationship between the cathode and anode in an electrolytic cell?

A: The cathode and anode are connected by an external power source, and they are the sites where reduction and oxidation occur, respectively. The cathode is the site where the reduction reaction takes place, and the anode is the site where the oxidation reaction takes place.

Q: What is the significance of the cathode in a nickel and copper electrolytic cell?

A: The cathode plays a crucial role in a nickel and copper electrolytic cell, as it is where the reduction reaction occurs. The reduction reaction involves the gain of electrons by the ions in the electrolyte, resulting in the formation of a solid product.

Q: What are the common mistakes to avoid when determining the cathode in an electrolytic cell?

A: Some common mistakes to avoid when determining the cathode in an electrolytic cell include:

Confusing the cathode and anode
Not understanding the reduction and oxidation reactions
Not considering the external power source
Not analyzing the electrolyte and electrodes

Q: How can I determine the cathode in a nickel and copper electrolytic cell?

A: To determine the cathode in a nickel and copper electrolytic cell, you need to:

Understand the reduction and oxidation reactions
Analyze the electrolyte and electrodes
Consider the external power source
Determine the site where reduction occurs

Conclusion

In conclusion, the cathode in a nickel and copper electrolytic cell is the electrode where reduction occurs, and it is the site where the reduction reaction takes place. The correct answer is A. $$Ni^{2+}$$ or B. $$Cu^{2+}$$. It is essential to understand the reduction and oxidation reactions, analyze the electrolyte and electrodes, and consider the external power source to determine the cathode in an electrolytic cell.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Brown, T. E., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, P. (2012). Chemistry: The Central Science (13th ed.). Pearson Education.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.