Oxidizing agent also known as the electron acceptor whereas Reducing agent known as the electron donor.
a) In this reaction, H2 is the electron donor and O2 is electron acceptor. Hence ,
Oxidizing agent = O2
Reducing agent = H2
b)In this reaction, Cu is the electron donor and HNO3 is electron acceptor. Hence
Oxidizing agent = HNO3
Reducing agent = Cu
5. Identify the oxidizing agent and reducing agent in each of the following: a) 2H2(g) +...
5&6 5) Identify the oxidizing agent, reducing agent, substance oxidized, and substance reduced. a) Consider the reaction Fe(NO3)3(aq) + H2S(aq) → FeS(s) + HNO3(aq) + S(s). b) Consider the reaction CuO(s) + H2(g) → Cu(s) + H2O(l). 6) Consider the reaction C(g) + O2(g) + CO2(g). (a) Determine the oxidation states of carbon and oxygen in CO2. (Drawing a Lewis struc- tures may help here.) (b) What are the oxidation states of the reactants carbon and oxygen? (c) Which substance...
The following reactions use the species above. Determine the oxidizing agent and the reducing agent, and which atom is oxidized or reduced for each reaction C2H4 + 3 O2 → 2 CO2 + 2 H2O Atom oxidized: Oxidizing agent: Atom reduced: Reducing agent: CuO + H2 → Cu + H2O Atom oxidized: Oxidizing agent: Atom reduced: Reducing agent: Cu + 4HNO3 → Cu(NO3)2 + 2 NO2 + 2 H20 Atom oxidized: Oxidizing agent: Atom reduced: Reducing agent:
Identify the substance that is being oxidized, reduced, the reducing agent a 2H2(g)+O2(g)--2H2O(g) Oxidized: Reduced: Oxidizing agent: Reducing agent:
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.
Identify the oxidizing and reducing agents for the following reaction (unbalanced equation): 12 (s) + NO3(aq) .......-> 103 (aq) + NO2 (g) (a)NO3 is reducing agent;12 is oxidizing agent (b) NO, is oxidizing agent; 12 is reducing agent (d) 12 is both reducing agent and oxidizing agent O O (c) NO, is both reducing agent and oxidizing agent
Identify the reduced substance, the oxidized substance, the reducing agent, and the oxidizing agent in the reaction of zinc with copper ions. Zn(s)+Cu2+(aq)⟶Zn2+(aq)+Cu(s)
Identify the oxidizing agent and the reducing agent on the reactant side of the following chemical equation. Then explain why you selected these compounds as the oxidizing agent and the reducing agent. MnO4 (aq) + SO2(aq) → MnO2(s) + 5042 (aq)
Lan contain viruses. Unless you need to edit, it's safer to stay in Protected View. Enable Editing 3. Write the equation for the nuclear reaction described in each of the following processes: a.Americium-241(241Am)undergoes alpha decay (inside a smoke detector) b.lodine-131 (131) undergoes normal beta decay (used in therapy for hyperthyroidism) C.Fluorine-18 (18F) undergoes positron emission (one of the radionuclides used in PET scans) 4. a) If an object that was once living died 35,500 years ago, what the exact percentage...
need to know what are the oxidizing agent and reducing agent Mno 4 (ap) + Fe 2+ 10 Mnoy (aq) + F e 2 (1) -) o Mnoi +204 + 2 ? ? - 4 Cr 2 O 7 st Noz (aq) - @ Cry 0,1 g + Fe or less 6 Noz tl y Acids I Part A Copper Nitrate 0 Cuss + He las Cu (s) + NO3-) ③ Cub) + NO3 Cay) = Solve for Balanced Net...
For the following redox reaction, identify the reducing agent and the oxidizing agent. Mn(s) + Fe2+ (aq) — Mn2+ (aq) + Fe(s) Reducing agent: x x. Hoo . Oxidizing agent: x x . He → J.