#15 Assign oxidation states to al the elements In this unbalanced reaction: Ag^+(aq) + Cu(s) rightarrow...
Assign oxidation states to all the elements in this unbalanced reaction: Ag+(aq) + Cu(s) --> Ag(s) + Cu2+ (aq) Which substance gets oxidized? Which substance gets reduced? Balance the Redox reaction.
For the following redox reaction: Cu(s) + HNO3(aq) → Cu2+(aq) + NO(g) a) Assign oxidation states to each of the elements in the reaction. b) Tell what is being oxidized, what is being reduced, what is the oxidizing agent and what is the reducing agent. c) Use the half-reaction method to balance the reaction as if it were taking place in acidic solution. d) Then balance the reaction as if it were taking place in basic solution. You do not...
6. For the following redox reaction: Cu(s) + HNO3(aq) + Cu(aa) + NO) a) Assign oxidation states to each of the elements in the reaction. b) Tell what is being oxidized, what is being reduced, what is the oxidizing agent and what is the reducing agent. c) Use the half-reaction method to balance the reaction as if it were taking place in acidic solution. d) Then balance the reaction as if it were taking place in basic solution. You do...
a Cu(s) + 2Ag+ (aq) → 2 Ag(s) + Cu2+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b HCl(g) + NH3 (g) → NH4Cl(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced c SiCl4 (l) + 2H2O(l) → 4HCl(aq) + SiO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d C14 (1) + 2Mg(s) + 2MgCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced e Al(OH)4-(aq) → AIO2- (aq) + 2H2O(l) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced
Consider the redox reaction Fe(s) + Cu2+ (aq) — Fe2+(aq) + Cu(s) Which substance gets oxidized? Which substance gets reduced? What is the reducing agent? What is the oxidizing agent?
Assign oxidation numbers to each of the elements in this unbalanced redox reaction. Cl2(g)+I^-(aq)--->Cl^-(aq)+IO3^-(aq)
[References] Sc(s) + 3Ag+ (aq) + 3 Ag(s) + Sc3+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced CE SC HBr(9) + NH3(g) + NH4Br(s) Redox? Oxidizing Agent in Reducing Agent Substance Oxidized Substance Reduced GeCl4 (1) + 2H2O(l) + 4HCl(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si C14 (1) + 2Ba(s) + 2BaCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes 2 SiBr, Ba SiBa Al(OH).-...
For the following reaction, (1) assign oxidation numbers for all the elements, (2) determine which one is oxidized and which one is reduced, and (3) balance the redox reaction in acidic solution. SO32–(aq) + MnO4–(aq) ® SO42–(aq) + Mn2+(aq)
Write a balanced overall reaction from these unbalanced half-reactions. Cu → cu2+ Ag+ → Ag balanced overall reaction: For a particular redox reaction NO is oxidized to NO3- and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional. Balance the following equation in basic conditions. Phases are optional.
Cu(s) + 4HNO3 --> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Cu2+(aq) + 4NH3(aq) --> [Cu(NH3)4]2+(aq) a. For each reaction, identify the oxidation number for each of the elements on both sides of the equation. b. Which of the reactions above is a redox reaction? Explain. c. Identify the element that is being reduced and the one that is being oxidized in the redox reaction. d. Identify the strong oxidizing agent and strong reducing agent in the redox reaction.