Explore BrainMass

Redox Reactions

Redox Reactions refer to a set of chemical reactions which consist of an electron transfer and a change in oxidation state of the reactant species. Redox is an abbreviated term for ‘reduction-oxidation’ reactions, where reduction refers to a gain of electron, while oxidation refers to a loss of electron.

In a reduction reaction, if an atom/molecule gains an electron, then its oxidation state will decrease. On the other hand, in an oxidation reaction, if an atom/molecule loses an electron, then its oxidation state will increase. The following redox reaction can be broken up into a reduction and oxidation reaction:

H_2 + F_2 --> 2HF

Oxidation reaction:
H_2 --> 2H+ +2e-

Reduction reaction:
F2 + 2e- --> 2F-

The overall redox reaction then involves the hydrogen transferring two electrons to the fluorine to create an ionic bond between the two atoms and forming the compound hydrogen fluoride (HF). Thus, understanding the basics of reduction and oxidation can help better grasp the complexities of some redox reactions.

Oxidation States of Manganese

I have done the lab and have submitted results. I am attaching a file with the procedures and the assignment. I have completed the 1st part of the Assignment, but I'm not sure how to do Parts 2 & 3. I really appreciate your help!

Electrochemistry and Redox/half reactions

Balance the following redox equations by the ion-electron method: 1) H2O2 + Fe2+ ---> Fe3+ + H2O (in acidic solution) CN- + MnO4- ---> CNO- + MnO2 (in basic solution) 2) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half cell reactions at 25 deg C. What is the equation for the cell reaction t

Redox and Ligand Substitution Chemistry of Cr(II) and Cr(III)

1.What are the Equations?: The redox processes in converting CrO3 to [Cr(H2O)5Br]2+. We dissolve chromium trioxide in acid to get CrO4(2-), and add that to a solution of hydrogen peroxide/perchloric acid. that should give [Cr(H2O)6]3+. This is then passed through a jones reductor into an perchloric acid/bromine solution to give

Balancing Redox Reactions

For the two unbalanced equation below -Write the unbalanced half-reactions. -Identify the species oxidized and the species reduced. -Identify the oxidizing agent and the reducing agent. -Balance the equation in acid. -Balance the equation in base. (a)H2O2(aq)+Ni^2+(aq) --> Ni^3+(aq) + H2O (b)Cr2o7^2-(aq) +Sn^2+(aq)

Cell Potentials and Balancing Redox Equations

Please see the attached file for the fully formatted problems. Question 1. In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reactio

Redox Reactions

This is a lab which deals with oxidation-reduction. We did a set of experiments in the lab. This is our procedure and observations: a) Dissolve a small amount of magnesium (II) chloride in half a beaker of water. (There is no redox process yet). Now add a few mL of NaOH. First make observations before the solution is stirred

Ionic Equations and Balancing Redox Reactions

1) Determine net ionic equations, if any, occurring when aqueous solutions of the following reactants are mixed. Select "True" or "False" to indicate whether or not the stated reaction (or "no reaction") correctly corresponds to the expected observation in each case. Magnesium chloride and sodium hydroxide; No reaction occu

Titrimetric Redox Determination of Iron in an Ore Using Dichromate

CHM 2290 Experiment #5 Titrimetric Redox Determination of Iron in an Ore Using Dichromate A. Introduction Many chemical compounds can be oxidized or reduced completely by reacting them with suitable reagents. Oxidation-reduction reactions can be utilized for quantitative determinations if a suitable means of detecting the eq

Redox and Electrochemistry

1.) Give the oxidation number of each element in the following: KIF4 2.) Is the following reaction a redox reaction? If yes, then what is the oxidizing agent and what is the reducing agent. 3NO3(g)+H20(l)-----2HNO3(aq)+NO(g) 3.) Write the balanced net ionic equation for the following reaction. Tell what subst

Oxidation and Reduction

1. Define the following concepts: a) oxidizing agent b) oxidized substance c) reducing agent d) reduced substance 2. Determine the oxidation numbers of the underlined elements in the following formulas: a) KClO3 b) NH4+ c) Cr2O72- d) MnO42- 3. Balance the following equations by the half-cell method.

How to Balance Redox Reactions

Balance the redox reaction: [Cr2O7]-2 + H2O2 ---> Cr3 + O2 When Zn + CoCl3 ---> ZnCl2 + CO is properly balanced, what is the total change in the number of electrons in zinc?

Understanding Redox Equations

Balance the redox equations and give the half-cell reactions and identify the oxidizing agent, species oxidized, reducing agent, and species reduced. In an acidic solution: CrO4^2-(aq)+ Cl-(aq)--> Cr^3+(aq) +HClO2(aq) In an acidic solution: Fe^2+(aq) + MnO4-(aq) --> Fe^3+(aq)+ Mn^2+(aq) In acidic solution: NH4+(aq) + NO3-(aq)


How do I balance an equation using the oxidation number method? Sn+HNO3---------->SnO2+NO2+H20

Redox equations

I need help understanding how to solve redox equations. If you could explain this to me in simple terms I would really appreciate it. i have a sample problem and can't even get past it. The problem is: K2CrO4 + Mg + HCl to CrCl3 + KCl + MgCl2 + h2O I need to know how to make a balanced equation out of this. Thank you very

Considering Oxidation and Reduction

Hi, I need some assistance understanding how to approach the following questions, 1) Assign oxidation numbers for each of the following atoms in the redox reaction given below. 2H^+(aq) + 2HNOsub2(aq) + 2I^- -> 2NO(g) +2H2O(l) +Isub2(s) a) Oxidation numbers for each. b) Which atom is being reduced and why. c) Which at

Redox Reaction Identified for an Atom

In each of the following reactions, identify the atom oxidized, the atom reduced, and balance the equation. 1. KBr + Fe2(SO4)3 -> Br2 + K2SO4 + FeSO4 2. Sn + HNO3 + H2O -> H2SnO3 + NO 3. Cu + AgNO3 -> Ag + Cu(NO3)2 Calculate the cell potential for each of the following reactions and determine whether the reaction is

Balance redox reactions

A) Acid Solution: KI+HNO3=KNO3+NO+I2+H2O Cr2O7<-2> + I<-> = Cr<+3> + IO3<-> b) MnO4<-> + Br<-> = MnO2 + BrO3<-> Bi(OH)3 + Sno2<-2> = Bi + SnO3<-2>

Redox Reaction: Ferrous Ion and Permanganate Ion

The ferrous ion, Fe2+(aq), reacts with the permanganate ion, MnO4- (aq), in an acidic solution to produce the ferric ion, Fe3+(aq). A 6.893 g sample of ore was mechanically crushed and tehn treated with concentrated hydrochloric acid, which oxidized all of the iron in the ore to the ferrous ion, Fe2+(aq). Next the acid solutio

Balancing redox equations by the oxidation number method

2KMnO4 + 5H2O2 + 6HCl --> 5O2 + 2MnCl2 + 8H2O + 2KCl I need to calculate the balanced NET IONIC equation for the above reaction. I've been using the oxidation number method and determined H2O2 is the reducing agent and KMnO4 is the oxidizing agent. Mn gained 5 electrons, but I'm not sure how many electrons Oxygen gained

Oxidizing and reducing agents

In the following reaction, identify the oxidizing and reducing agents. Br2 + H2 --> 2HBr a. H+ is the reducing agent, Br- is the oxidizing agent b. Br2 is the reducing agent, H+ is the oxidizing agent c. Br2 is the reducing agent, H2 is the oxidizing agent d. HCl is the reducing agent, Br2 is the oxid

Redox reaction in acidic solution

I need to separate these into half reactions, and indicate the changes in oxidation state, then give the overall equation. First I put water into a test tube, then I added potassium permangate. Next I added sulfuric acid, and after mixing that together I also added potassium iodide. I understand how to balance redox equ