In the following oxidation-reduction chemical reaction which chemical species is getting reduced? Hint: Oxygen oxidation number is -2 in Cr20,2 (aq) and -1 in H2O2(aq) and O in O2@)· Hydrogen oxidation number is +1. O2 + Cr3+, * (aq) → H2O2(aq) + Cr20,2 (aq) O Cr3+ and Cr20,2- H2O2 and Cr2072- Cr3+ and H2O2 none of them O2 and Cr3+

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --

+ 1.14 V TI Pt Cr3+ (1 M) Cr2 (1 M) T13+ (1 M) T13+ (aq) + 3e-→ TI (s) Cr2+ (aq) → Cr3+ (aq) + e- What happens to the thallium electrode as the redox reaction progresses? O it gains mass as thallium metal is plated onto the electrode O it loses mass as the thallium metal is consumed by the reaction O it spontaneously ignites and burns O the thallium electrode is inert and unaffected by the redox reaction O a thick layer of thallium salt develops on the clectrode DELL

When the following skeletal equation is balanced under acidic conditions, what are the coefficients of the species shown? | C103 + |Mn²+ CI + |MnOq Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of - (Enter 0 for neither.) Which species is the oxidizing agent?