Oxidation-reduction reactions (often called \"redox\" for short) are reactions t
ID: 587028 • Letter: O
Question
Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. Oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. In general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. An oxidizing agent is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction. A reducing agent is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction. As a summary, keep in mind the following: Oxidation means an increase in oxidation state and a loss of electrons and involves a reducing agent. Reduction means a decrease in oxidation state and a gain of electrons and involves an oxidizing agent. Part A Which element is oxidized in this reaction? Fe2O3+3CO2Fe+3CO2 Enter the chemical symbol of the element. Hints C is oxidized SubmitMy AnswersGive Up Correct Carbon gets oxidized in the process of reducing iron. Iron gets reduced in the process of oxidizing carbon. Part B Which substance is the oxidizing agent in this reaction? Fe2O3+3CO2Fe+3CO2 Part C Which element is reduced in this reaction? 16H++2Cr2O72+C2H5OH4Cr3++11H2O+2CO2 Enter the chemical symbol of the element.
Explanation / Answer
Answer:-
For Fe2O3 + 3CO ------------> 2Fe + 3CO2
The element oxidised = C
Fe2O3 + 3CO ------------> 2Fe + 3CO2
Oxidising agent = Fe2O3
16H+ + 2Cr2O72- + C2H5OH --------------> 4Cr3+ + 11H2O + 2CO2
The element which is reduced = Cr
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