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Decomposition Reactions - Redox Reactions Video Lecture - Class 11
FAQs on Decomposition Reactions - Redox Reactions Video Lecture - Class 11
| 1. What is a decomposition reaction? |  |
Ans. A decomposition reaction is a type of chemical reaction in which a compound breaks down into simpler substances. It is the opposite of a synthesis reaction, where simpler substances combine to form a more complex compound.
| 2. How do decomposition reactions occur? | |
Ans. Decomposition reactions occur when a compound is heated, exposed to light, or reacts with another substance. These factors provide the necessary energy to break the bonds within the compound, leading to the formation of simpler substances.
| 3. What are some examples of decomposition reactions? | |
Ans. Some examples of decomposition reactions include the breakdown of hydrogen peroxide into water and oxygen gas, the decomposition of calcium carbonate into calcium oxide and carbon dioxide gas, and the decomposition of ammonia into nitrogen gas and hydrogen gas.
| 4. What are redox reactions? | |
Ans. Redox reactions, also known as oxidation-reduction reactions, are chemical reactions that involve the transfer of electrons between reactants. One reactant undergoes oxidation by losing electrons, while the other undergoes reduction by gaining electrons.
| 5. Can decomposition reactions be classified as redox reactions? | |
Ans. Yes, decomposition reactions can be classified as redox reactions if there is a transfer of electrons involved. For example, the decomposition of hydrogen peroxide into water and oxygen gas is a redox reaction because the hydrogen peroxide molecule loses electrons (oxidation) while the oxygen molecule gains electrons (reduction).
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Nov 22, 2024 Last updated |
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