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Oxidation and Reduction Chemical Reactions Video Lecture | Extra Documents, Videos & Tests for Class 10
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FAQs on Oxidation and Reduction Chemical Reactions Video Lecture - Extra Documents, Videos & Tests for Class 10
| 1. What is oxidation and reduction in chemical reactions? |  |
Ans. Oxidation is the process in which a substance loses electrons, resulting in an increase in its oxidation state. Reduction, on the other hand, is the process in which a substance gains electrons, leading to a decrease in its oxidation state. In chemical reactions, oxidation and reduction always occur together and are referred to as redox reactions.
| 2. How can oxidation and reduction be identified in a chemical reaction? | |
Ans. Oxidation and reduction can be identified by analyzing the changes in the oxidation states of the elements involved in the reaction. If the oxidation state of an element increases, it undergoes oxidation, whereas if the oxidation state decreases, it undergoes reduction. Additionally, the transfer of electrons from one element to another is another indicator of oxidation and reduction.
| 3. Why are oxidation and reduction important in chemical reactions? | |
Ans. Oxidation and reduction are important in chemical reactions because they involve the transfer of electrons, which is crucial for the formation or breaking of chemical bonds. These reactions play a vital role in various natural processes, such as respiration, photosynthesis, corrosion, and combustion. They are also utilized in industries for the production of chemicals, fuels, and metals.
| 4. What are some examples of oxidation and reduction reactions? | |
Ans. Some examples of oxidation reactions include the rusting of iron (Fe), the combustion of fuels like gasoline, and the reaction of magnesium (Mg) with oxygen (O2) to form magnesium oxide (MgO). Examples of reduction reactions include the conversion of iron(III) oxide (Fe2O3) to iron (Fe) using carbon monoxide (CO) in the blast furnace and the reduction of silver ions (Ag+) to silver metal (Ag) using zinc (Zn) in a displacement reaction.
| 5. How can oxidation and reduction reactions be balanced? | |
Ans. To balance oxidation and reduction reactions, it is necessary to ensure that the number of atoms and the total charge are conserved. This can be achieved by adjusting the coefficients of the reactants and products in the chemical equation. The balancing process involves identifying the elements undergoing oxidation and reduction, balancing the atoms other than oxygen and hydrogen first, balancing oxygen atoms using water molecules, and finally balancing hydrogen atoms using hydrogen ions or protons.
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Nov 19, 2024 Last updated |
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