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# Redox Reactions

### Redox titration

Please help with balencing this equation I am trying to get the half reaction balenced first FeCl2+Kmno4+HCL------------>FeCL#+KCL+MnCL2 +H2 Fecl2------------->Fecl3 now what?

### 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

### Balancing Half-Cell Reactions

Balance both equations by the half-cell method, showing both half-cell reactions and identifing them as oxidation or reducton. a. Cl2(g)+ OH- <--> Cl- + ClO3- + H20(l) b. SO4- + I- + H+ <--> S2- + I2(g) + H2O(l)

### 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>

### Balance redox that occur in basic using 1/2 reaction method

3a) Balance the oxidation-reduction reactions that occur in basic solution using half-reaction method Al(s) + MnO4<-> (aq) = MnO2(s) + Al(OH)4<->(aq) 3b) Same method: NO2<-> (aq) + Al(s) = NH3(g) + AlO2<->(aq)

### Balance redox in acidic solution using half reaction

2 a) Balance the following Oxidation-reduction reactions that occur in acidic solution using half reaction method and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced Mn<2+>(aq) + NaBiO3(s) = Bi<3+> (aq) + MnO4<->(aq) 2 b) Same method: Cu(s) + NO3<-> (aq) = Cu

### 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

### Step-wise procedure for balancing redox reactions

Balance the following redox reaction: MnO4-(aq) + C2O42-(aq) -> Mn2+(aq) + CO2(g)