17.27c | Calculate a corresponding standard free energy change (kJ) from −2.439 V and n = 1

(1:17)

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

(5:34)

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

(11:2)

17.22c | Calculate the standard cell potential for Mn(s) + Ni2+(aq) → Mn2+(aq) + Ni(s)

(7:35)

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

(10:14)

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

(5:21)

How to Balance Redox Equations in Basic Solution

(18:)

17.47c | How long would it take to reduce 1 mole of Cr5+ using a current of 37.45 A

(5:46)

17.22b | Calculate the standard cell potential for 3Cu2+(aq) + 2Al(s) → 2Al3+(aq) + 3Cu(s)

(6:2)

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

(16:40)

17.24 | Determine the cell reaction and standard cell potential at 25 °C for a cell made from a

(10:2)

17.43 | If a 2.5 A current flows through a circuit for 35 minutes, how many coulombs of charge moved

(5:20)

17.11d | Write a cell schematic for 3CuNO3(aq) + Au(NO3)3(aq) → 3Cu(NO3)2(aq) + Au(s)

(12:53)

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

(6:45)

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

(4:39)

18.5 cell potential, free energy, and equilibrium constant

(9:)

16.21g | How to calculate ΔS° for Zn(s) + CuSO4(s) → Cu(s) + ZnSO4(s)

(5:11)

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

(7:35)

16.17c | Predict the sign of the entropy change: 2C6H14(l) + 19O2(g) → 14H2O(g) + 12CO2(g)

(5:55)

21.14a | How to balance a nuclear equation: Li-7 + ? → 2He-4

(5:18)

17.32d | Suppose sulfuric acid is added to the half-cell with the lead electrode and some PbSO4(s)

(9:13)

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

(11:52)

17.28b | Calculate a corresponding standard cell potential from −45 kJ/mol, n = 1

(5:49)

17.28a | For each pair of standard free energy change and electron stoichiometry values below

(6:19)

16.3d | Is a ball thrown into the air spontaneous or nonspontaneous?

(2:41)

17.3d | Write a balanced equation for the overall reaction: Ag → Ag+ + e−, MnO4− + 4H+ + 3e− → MnO2

(5:47)

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

(11:49)