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Rank these species by their ability to act as an oxidizing agent. Br2, Pb2+, Mg2+, Cr3+
Which is the strongest oxidizing agent? O Ags) Cu(s) Mg(s)
Rank these species by their ability to act as an oxidizing agent Cu+ Br2 Cr2+ Na+
Which of the following is the strongest oxidizing agent? 6 Cl2(g) + 2€ - 2 C1-(29) Cut(aq) + € - Cu(5) 5042-(29) + 4H+ (aq)+26 - H2SO3(aq) + H2O(1) MnO4+(29) + 4 H+ (aq) +3 e - MnO2(s) + 2 H2O(1) EP1.36 V EP0.52V E° -0.20 V E1.68 V 9 -- MnO2(s) 5042-(aq) 12 Cu*(aq) MnO4 (aq) 15 ci (aq) 18
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...
A. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Sn2+(aq) + 2e-Sn(s) -0.140V Cr3+(aq) + 3e-Cr(s) -0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cl2(g) oxidize Cr(s) to Cr3+(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank. B. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Cu2+(aq) + 2e-Cu(s) 0.337V Mn2+(aq) + 2e-Mn(s) -1.180V (1) The...
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...
Which of the following is the strongest oxidizing agent? MnO4 ̄ (aq) + 4 H+ (aq) + 3 e ̄ → MnO2 (s) + 2 H2O (l) I2(aq) +2e ̄ →2I ̄(aq) Zn2+(aq) +2e ̄ →Zn(s) εo = 1.68 V εo =0.54V εo =-0.76V Al Ni Both Al and Ni would work Neither Al nor Ni would work
2 Fe + N2 + 4 H2O 2 Fe(OH)2 + N2H4 For the above redox reaction, assign oxidation numbers and use them to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent:
Oxidizing agent Reducing agent termine which half-cell elect the potentials, note that are them is to note that Pb the more negative reductie + 2e Ph. The half en offis reversed. iting both potentials: 14. Mno + SO, + HO SO M hali Oxidation Half Reaction: Reduction: Cu Oxidation Pb Reduction Hall Reaction: the reaction with respect either (or both) half rea te in both half reactions Add the two half-rear Oxidizing agent: Reducing agent + 15. 10. + HSO,...