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OXIDATIONREDUCTION REACTIONSIn this experiment, you will perform a series of redox reactions. You will identify the oxidizing and reducing agents and the products in each reaction based on your observations.
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01
Balance the atoms in the equation by adding coefficients
02
Identify the oxidation numbers of each element in the reaction
03
Determine which elements are being oxidized and which are being reduced
04
Add electrons to balance the changes in oxidation numbers
05
Ensure that the number of electrons lost in the oxidation half-reaction is equal to the number of electrons gained in the reduction half-reaction
06
Add the balanced half-reactions together to form the overall redox reaction

Who needs redox reactions - examples?

01
Chemists use redox reactions to understand and predict chemical reactions
02
Environmental scientists use redox reactions to study the behavior of pollutants in soil and water
03
Industrial engineers use redox reactions in the production of chemicals and materials
04
Students studying chemistry need to understand redox reactions for their coursework and exams

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Redox reactions, or reduction-oxidation reactions, are chemical processes involving the transfer of electrons between two species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Examples include the rusting of iron (Fe oxidizes to Fe2O3) and the reaction between hydrogen and oxygen to form water (2H2 + O2 -> 2H2O).
Individuals or organizations involved in chemical manufacturing, pharmaceuticals, and environmental monitoring that handle substances undergoing redox reactions may be required to file relevant reports. For example, chemical companies might file documentation related to their processes involving oxidation and reduction.
Filling out redox reactions typically involves documenting the conservation of mass and charge, identifying oxidation states, and balancing the overall equation. This includes writing half-reactions for the oxidation and reduction processes. An example would be balancing the redox reaction of potassium permanganate (KMnO4) in acidic medium.
The purpose of redox reactions is to facilitate energy transfer, synthesize compounds, and drive various biochemical processes. Examples include cellular respiration (glucose oxidation to produce ATP) and photosynthesis (conversion of carbon dioxide and water to glucose and oxygen through reduction).
Reports on redox reactions should include the substances involved, their oxidation states, balanced equations, and the conditions under which the reactions occur. For example, a report may include the details of a redox reaction between iron and copper sulfate, specifying the reactants and products.
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