Class 11 chemistry redox reaction exercise solutions

Redox reaction exercises online

+VI -II +IV -II +VI -II +III Cr2O72- + SO32- ⇢ SO42- + Cr3+↓+IV -II +VI -II Oxidation: SO32- → SO42- + 2 e- +VI -II +IIIReduction: Cr2O72- + 6 e- → 2 Cr3+↓Oxidation: SO32- → SO42- + 2 e- Charge: 2 - → 4 - Reduction: Cr2O72- + 6 e- → 2 Cr3+Charge: 8 - → 6 + ↓Oxidation: SO32- → SO42- + 2 e- + 2 H+ Reduction: Cr2O72- + 6 e- + 14 H+ → 2 Cr3+(reaction in acidic environment)↓Oxidation: SO32- + H2O → SO42- + 2 e- + 2 H+ | - 3 Reduction: Cr2O72- + 6 e- + 14 H+ → 2 Cr3+ + 7 H2O | - 1 ↓Cr2O72- + 6 e- + 14 8 H+ + 3 SO32- + 3 H2O → 2 Cr3+ + 7 4 H2O + 3 SO42- + 6 e- + 6 H+↓Cr2O72- + 3 SO32- + 8 H+ → 3 SO42- + 2 Cr3+ + 4 H2O

Redox reactions exercises difficult

Substances that release oxygen are oxidizing agents. They are reduced by the release of oxygen.An oxidizing agent is a substance that can release oxygen to other substances and thereby oxidize these reaction partners.In such chemical reactions, oxidation and reduction can no longer be separated from each other, both occur simultaneously.One substance is deprived of oxygen, it releases it - this is called reduction. At the same time, the other substance absorbs oxygen - this is called oxidation.Oxidation and reduction represent an inseparable unit.A chemical reaction in which oxidation and reduction occur simultaneously is called a redox reaction.

Redox reaction in the broader sense Electron donors Redox reaction Reducing agent Electron acceptors Reduction Redox reactions Oxidation Redox reaction in the narrower sense Oxidation number Oxidizing agent

Redox reactions exercises easy

In the thermite reaction, the substance that gives up electrons is the metal aluminum, which is oxidized. In our example, the substance that accepts electrons is the iron(II) ion ($\ce{Fe^{2+}}$) in the iron oxide, which is reduced.

$\begin{array}{lclclcl} 2\, \overset{\color{#669900}\text{0}}{\ce{Al}} & + & 3\, \overset{\color{#669900}\text{+II~-II~~}}{\ce{FeO}} & \longrightarrow & 2\, \overset{\color{#669900}\text{0}}{\ce{Fe}} & + & 2\, \overset{\color{#669900}\text{+III~-II~~}}{\ce{Al2O3}} \end{array}$

The result is: two aluminum react to form two aluminum triples, donating a total of 6 electrons. On the other hand, three iron two-ipluses react to give three iron with a total of 6 electrons. Now we have the same number of electrons in both partial equations.

Redox reactions exercises uni

1. the alkali metals 2. the reaction of the alkali metals with water 3. the oxyhydrogen test 4. the alkaline earth metals 5. the reaction of the alkaline earth metals with water 6. the halogens 7. the reaction of sodium with chlorine 8. the reaction of aluminum with bromine 9. the formation of salts 10. the noble gases

1. the different atomic models (1) 2. the different atomic models (2) 3. the Rutherford scattering experiment (1) 4. the Rutherford scattering experiment (2) 5. around atom, proton, neutron and electron (1) 6. the atom, proton and neutron (2) Around atom, proton, neutron and electron (2) 7. shell occupancy of different atoms 8. spherical cloud models and lewis notation (1) 9. spherical cloud models and lewis notation (2) 10. ion formation - production of common salt (NaCl)

1. the Daniell element 2. the Leclanché element - the zinc-carbon battery 3. the alkaline-manganese battery 4. the zinc-air button cell 5. the lead accumulator (1) 6. the lead accumulator (2) 7. the nickel-metal hydride accumulator (1) 8. the nickel-metal hydride accumulator (2) 9. the lithium ion accumulator (1) 10. the lithium ion accumulator (2)