1. Distinguish between a conductor and electrolyte.
2. State Faraday's first law of electrolysis
3. What is an electrochemical cell
4. State five differences between an electrochemical cell and electrolytic cell.
1. A substance which conducts electricity (ion, e) in only molten form is called electrolyte.
A substance which has ability to conduct electric current either in molten or in solid state is called a conductor.
Every electrolyte is a conductor but not every conductor is an electrolyte.
2. Faraday's first law of electrolysis States that '' Mass of a substance liberated or deposited during Electrolysis is proportional to the quantity of electricity passed through the solution ''.
3. An electrochemical cell is a device capable of either generating electrical energy from chemical reactions or using electrical energy to cause chemical reactions.
4. In electrochemical cell ( Salt is required. Cathode is the positive electrode. Anode is the negative electrode. Two electrolytes are required. Electrodes are in separate compartments) In Electrolytic cell ( Salt bridge is not required. Cathode is the negative electrode. Anode is the positive electrode. Only one electrolyte is required. Electrodes are in the same compartment)
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1. To distinguish between a conductor and an electrolyte, we need to consider their behavior in conducting electricity.
Conductor: A conductor is a material that allows electric current to flow through it easily. It has a high number of free electrons that are able to move within the material when a potential difference is applied. Examples of conductors include metals like copper, silver, and aluminum.
Electrolyte: An electrolyte is a substance that conducts electricity when dissolved in water or molten form. It undergoes a process called ionization, where it breaks down into positive and negative ions. These ions can move and conduct electricity through the solution. Examples of electrolytes include salts like sodium chloride (NaCl) and acids like hydrochloric acid (HCl).
In summary, the key difference is that conductors conduct electricity due to the movement of free electrons, while electrolytes conduct electricity due to the movement of ions.
2. Faraday's first law of electrolysis states that the amount of substance produced or consumed at an electrode during electrolysis is directly proportional to the quantity of electric charge passing through the electrolyte. Mathematically, it can be expressed as:
m = ZQ
Where:
- m is the mass of the substance produced or consumed
- Z is the electrochemical equivalent, a constant specific to each substance
- Q is the total electric charge passed through the electrolyte
This law indicates that the amount of substance involved in an electrolytic reaction is determined by the quantity of electric charge passing through the system.
3. An electrochemical cell is a device that converts chemical energy into electrical energy through redox reactions. It consists of two electrodes, an electrolyte, and a separator. The electrodes are typically made of conductive materials, and the electrolyte is a solution or paste that allows the flow of ions. The separator prevents direct contact between the electrodes, while still allowing ion transfer.
Electrochemical cells can be divided into two types, based on their operation:
- Galvanic (voltaic) cells: These cells generate electrical energy from spontaneous redox reactions. The chemical energy of the reactants is converted into electrical energy. Examples of galvanic cells include batteries.
- Electrolytic cells: These cells use electrical energy to drive non-spontaneous redox reactions. Electrical energy is converted into chemical energy as the reaction takes place. Electrolytic cells are commonly used in processes like electroplating and electrolysis.
4. Here are five differences between an electrochemical cell and an electrolytic cell:
1. Power Source: In an electrochemical cell, the redox reaction occurs spontaneously, generating electrical energy. It does not require an external power source. Conversely, an electrolytic cell requires an external source of electrical energy to drive the non-spontaneous reaction.
2. Redox Reaction Direction: In an electrochemical cell, the reaction proceeds spontaneously in one direction, from anode to cathode. However, in an electrolytic cell, the reaction is forced to occur in the opposite direction by applying an external potential difference.
3. Cell Operation Mode: Electrochemical cells operate in a closed system, meaning the reactants are consumed, and the cell eventually becomes inactive. Conversely, in an electrolytic cell, the cell operates in an open system, allowing the reactants to be continuously replenished.
4. Energy Conversion: Electrochemical cells convert chemical energy into electrical energy, which can be used to power devices. In contrast, electrolytic cells convert electrical energy into chemical energy, resulting in the production of substances or the deposition of metals.
5. Electrode Polarity: In an electrochemical cell, the anode is typically associated with oxidation, and it has a negative charge. The cathode is associated with reduction and has a positive charge. In an electrolytic cell, the polarity is reversed, with the anode being positive and the cathode negative, due to the direction of the externally applied potential difference.