a. Fe^3 + is oxidized. b. Fe^3 + increases in oxidation number. c. Fe^3 + is red

Question

a. Fe^3 + is oxidized. b. Fe^3 + increases in oxidation number. c. Fe^3 + is reduced. d. F is reduced. In the chemical reaction, Zn (s) + CuSO4 (aq) rightarrow ZnSO4 + (aq) + Cu (s) a. metallic zinc is the reducing agent. b. metallic zinc in reduce. c. copper ion is oxidized. d. sulfate ion is the oxidizing agent. In this reaction, which substance behaves as the oxidizing agent? Pb + PbO2 + 2H2SO4 rightarrow 2PbSO4 + 2H2O a. Pb b. PbSO4 c. PbO2 d. H2SO4 In which group can each substance act as an oxidizing agent? a. Cl_2, MnO_2, Cu b. Cl_2, MnO^4 -, Cu^2 + c. Cl^-, MnO^4 -, Cu^+ Which of the following net ionic equation best represent the reaction that takes place in aqueous solution, when sulfuric acid and sodium hydroxide solution are mixed? a. H_2SO4 + 2OH rightarrow SO_3^2- + 2H_2O b. H^+ + NaOH rightarrow Na^+ + H_2O c. H^+ + OH doubleheadarrow H_2O

Explanation / Answer

Q18.

oxidizing agent --> Contains the species reducing

therefore

Pb goes from 0 to +2, it loses 2 electrons, therefore, it is gettind oxidized

therefore, it is the REDUCING agent, so we can't choose Pb

PbO2 --> Pb goes from +4 to +2, it gains 2 electrons, it is reducing

it contians the REDUCING species, so it must be the oxidizing agent

this is our answer

note that H2SO4 can't be since H, S and O won't change oxidation states

best answer is then PbO2

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