What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: Cr2O72-(aq) + 6X2+(aq) + 14H+(aq) → 2Cr3+(aq) + 6X3+(aq) + 7H2O(l)

Identify the oxidizing agent and draw tie-lines to determine the reducing and oxidizing agents for the following reaction: 10 HNO3 (aq)  + I2 (s)  → 2 HIO3 (aq) + 10 NO2 (g)  +  4 H2O (l)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H 2C 2O 4 and H 2O in the balanced reaction? MnO 4⁻( aq) + H 2C 2O 4( aq) → Mn 2+( aq) + CO 2( g)     H2C2O4 = 5, H2O = 8     H2C2O4 = 1, H2O = 4     H2C2O4 = 5, H2O = 1     H2C2O4 = 1, H2O = 1     H2C2O4 = 3, H2O = 2

In the following redox equation, choose the correct oxidation half equation: 6 103 (aq) + Br (aq) → Br2 (1) + IBr(s) O 103 (aq) + 4 e + IBr(s) Br2 (1) +2e +Br" (aq) 2Br" (aq) + Br2 + 2e (1)

In the following redox reaction what is being oxidized and what is being reduced? S2O82–(aq) + 2H+(aq) + 2I–(aq) → 2HSO4–(aq) + I2(aq)

Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction

Identify the oxidizing and reducing agents in the following: 2MnO4−(aq) + 10 Cl−(aq) + 16 H+(aq) → 5 Cl2(g) + 2 Mn2+(aq) + 8 H2O(l)

Please answer the following question:

Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) Which species is the reducing agent? HCI H2 MgCl2 Mg

Consider the same chemical equation: 14 H+(aq) + 6Fe2+(aq) + Cr2O72-(aq) ⟶ 6Fe3+(aq) + 2Cr3+(aq) + 7H2O(l) How many electrons are being transferred in this redox reaction?