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

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

(1:27)

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

(6:19)

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

(5:34)

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

(6:29)

17.20 | The masses of three electrodes (A, B, and C), each from three different galvanic cells, were

(6:11)

Cell Potential Problems - Electrochemistry

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12.24 | How to determine the rate law, the rate constant, and the order order of a reaction

(14:45)

17.38 | Consider the following metals: Ag, Au, Mg, Ni, and Zn. Which of these metals could be used

(9:57)

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

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12.74 | Experiments were conducted to study the rate of the reaction represented by this equation

(40:5)

12.62 | Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2

(12:20)

Concentration Cells \u0026 Cell Potential Calculations - Electrochemistry

(14:22)

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

(5:30)

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)

17.32b | What are the reactions at the anode, cathode, and the overall reaction?

(5:22)

16.46 | Determine the normal boiling point (in kelvin) of dichloroethane, CH2Cl2. Find the actual

(17:16)

17.32c | Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could

(4:30)

17.27a | For each pair of standard cell potential and electron stoichiometry values below, calculate

(5:20)

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

(7:35)

17.36 | Using the information thus far in this chapter, explain why battery-powered electronics

(4:39)

12.36 | What is the half-life for the first-order decay of phosphorus-32? (32 P → 32 S + e−) The

(5:28)

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

(5:21)

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

(8:25)

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

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17.33c | If a particular dead battery was found to have [Cu2+] = 0.11 M, what was the concentration

(5:24)

17.32a | Consider a battery made from one half-cell that consists of a copper electrode in 1 M CuSO4

(8:23)