17.21b | Calculate the standard cell potential for 2Ag+(aq) + Cu(s) → Cu2+(aq) + 2Ag(s)

(4:59)

17.21b | Calculate the standard cell potential for 2Ag+(aq) + Cu(s) → Cu2+(aq) + 2Ag(s)

(1:51)

17.21a | Calculate the standard cell potential for Mg(s) + Ni2+(aq) → Mg2+(aq) + Ni(s)

(6:29)

17.21c | Calculate the standard cell potential for Mn(s) + Sn(NO3)2(aq) → Mn(NO3)2(aq) + Sn(s)

(7:35)

17.21d | Calculate the standard cell potential for 3Fe(NO3)2(aq) + Au(NO3)3(aq) → 3Fe(NO3)3(aq) +

(8:25)

4.20a | Identify the atoms that are oxidized and reduced: Mg(s) + NiCl2(aq) → MgCl2(aq) + Ni(s)

(12:7)

17.6d | Balance the equation in an basic solution: Al(s) + CrO42−(aq) → Al(OH)3(s) + Cr(OH)4−(aq)

(18:34)

17.16b | The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a

(10:6)

17.2a | Identify the half-reaction either oxidation or reduction: Cl− → Cl2

(5:1econd)

7-7 MINIMUM WIRE-BENDING SPACE - 408.3(G)

(3:44)

17.49 | An irregularly shaped metal part made from a particular alloy was galvanized with zinc using

(16:40)

17.11c | Write a cell schematic for Mn(s) + Sn(NO3)2(aq) → Mn(NO3)2(aq) + Sn(s)

(10:14)

Trick to identify Anode and Cathode in a cell reaction

(3:35)

17.11a | Write a cell schematic for Mg(s) + Ni2+(aq) → Mg2+(aq) + Ni(s)

(6:45)

17.31b | Calculate the equilibrium constant for CdS(s) ⇌ Cd2+(aq) + S2−(aq) using cell potentials

(11:52)

Electrochemistry (Cell Potential \u0026 Free Energy )

(10:45)

17.31c | Calculate the equilibrium constant for Hg2+(aq) + 4Br−(aq) ⇌ [HgBr4]2−(aq) using E values

(11:2)

17.47b | How long would it take to reduce 1 mole of Ca2+ using a current of 2.22 A

(5:21)

17.48 | A current of 2.345 A passes through the cell shown in Figure 17.19 for 45 minutes. What is

(18:32)

17.27b | Calculate a corresponding standard free energy change (kJ) from +0.434 V and n = 2

(5:34)

`2Ag^(+)(aq) + Cu(s) rightarrow Cu^(2+)(aq) + 2Ag(s)` The standard potential

(2:46)

17-28 (b) WIRING METHODS – CONDUCTOR BENDING RADIUS - 300.34 AND 314.71

(1:48)

17.47d | How long would it take to reduce 1 mole of Au3+ using a current of 3.57 A

(4:39)

17.31a | Calculate the equilibrium constant for AgCl(s) ⇌ Ag+(aq) + Cl−(aq) using cell potentials

(11:49)

17.6a | Balance the equation in an basic solution: SO32−(aq) + Cu(OH)2(s) → SO42−(aq) + Cu(OH)(s)

(20:28)