17.12b | Identify the half-cell reactions for Ni(s) │ Ni2+(aq) ║ Ag+(aq) │ Ag(s)

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17.12b | Identify the half-cell reactions for Ni(s) │ Ni2+(aq) ║ Ag+(aq) │ Ag(s)

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17.12a | Identify the half-cell reactions for Mg(s) │ Mg2+(aq) ║ Cu2+(aq) │ Cu(s)

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

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12.5a | Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0

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A voltaic cell consists of an Au electrode and a Cu electrode Calculate Au3+ if Cu2+=1.20M and E

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A voltaic cell prepared using aluminum and nickel has the following cell notation Als | Al3+aq ||

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17.2c | Identify the half-reaction either oxidation or reduction: H2 → H+

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

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

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

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17.10 | Why must the charge balance in oxidation-reduction reactions?

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

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12.15b | How would increasing the concentration of CO from 0.01 M to 0.03 M affect the rate of

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

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