12th Grade CBSE Electrochemistry Concepts Quiz

11 Questions

What factor determines the amount of a substance deposited or dissolved during electrolysis?

The quantity of electric charge passed through the solution

In electrolysis, what happens when a steady direct current is passed through a conducting solution containing metal salts?

Metal deposits itself onto the negative electrode

What do cathodically acting nonmetallic elements take up from the acid medium in electrolysis?

Hydrogen gas

What are some practical implications of electrochemistry mentioned in the text?

Waste management technologies based on ion exchange resins

How do students benefit from studying electrochemical theory according to the text?

By learning about various industrial applications such as nuclear reactors and fuel cells

What occurs during oxidation in a redox reaction?

An element loses electrons

Which process involves the transfer of electrons from one atom to another?

Redox reaction

What is the main difference between Galvanic and Voltaic cells?

Galvanic cells require an external energy source

Which of the following is NOT an example of a redox reaction?

Photosynthesis in plants

What happens during reduction in a redox reaction?

An element gains electrons

How do Galvanic cells and Voltaic cells differ in terms of energy requirements?

Galvanic cells require an external energy source, Voltaic cells produce their own energy

Study Notes

Electrochemistry is a fascinating branch of chemistry that focuses on the relationship between chemical reactions and electricity. In this context, we will explore some key concepts related to electrochemistry in the 12th grade curriculum under the Central Board of Secondary Education (CBSE) board.

Redox Reactions

Redox reactions are essential to understanding many phenomena in electrochemistry. A redox reaction involves the transfer of electrons from one atom to another. Oxidation occurs when an element loses electrons while reduction happens when it gains electrons. These processes can also occur within molecules if they have multiple atoms with different valence states. Some common examples of redox reactions include rusting iron, corrosion, and cellular respiration in living organisms like plants and animals where glucose reacts with oxygen to form carbon dioxide and water.

Galvanic Cells and Voltaic Cells

Galvanic cells produce electrical currents through spontaneous oxidation and reduction reactions, which generate potential difference. This creates an electric field around the cell. Voltaic cells work similarly but require an external source of energy to maintain the cell's output voltage. Both types of cells help us understand how batteries function, as well as other applications such as fuel cells.

Faraday’s Laws of Electrolysis

Faraday's laws of electrolysis state that the amount of a substance deposited or dissolved during electrolysis depends on the quantity of electric charge passed through the solution containing the substance. For example, when you pass a steady direct current through a conducting solution containing metal salts, the metal deposits itself onto the negative electrode until all of the positive charges needed by the cations involved are neutralized. Conversely, cathodically acting nonmetallic elements take up hydrogen gas from the acid medium present.

Electrochemistry has numerous practical implications beyond academia. It forms the basis for modern life sciences such as biochemistry, waste management technologies based on ion exchange resins, and solar power generation using photovoltaic devices. By studying these principles, students gain insights into various industrial applications of electrochemical theory – including nuclear reactors and fuel cells.