Determine the Q expression for the following unbalanced redox reaction: 2+ Zn + Ag → Zn²+ + Ag The standard reduction potentials are: Age → Ag Zn²+ + 2e → Zn 2+ a) Q = ObQ= d) +12 [Ag+]² [Zn²+] [Ag+] [Zn²+] [Zn²+] Q=Ag¹12 2+ [Zn²+] E = +0.80 V E-0.76 V

Given the following standard reduction potentials, E°red, which species has the  greatest tendency to be oxidized? S (s) + 2 H+ + 2e−    → H2S (g)            E°red = +0.144 V O2 (g) + 4 H+ + 4e− → 2 H2O (l)         E°red = +1.229 V Sn2+ (aq) + 2e−        → Sn (s)              E°red = −0.137 V   HERE ARE THE OPTIONS: O2 (g) S (s) Sn (s) H2S (g)

Given the following standard reduction potentials, determine K for the following reaction at 25°C.  Report your answer to 3 significant figures in scienitific notation using the format of 6.022E23 for 6.022 × 1023. Pb2+(aq) + SO42−(aq) → PbSO4 (s)     E°red Pb2+(aq) + 2e− → Pb (s)   -0.126 V PbSO4 (s) + 2e− → Pb (s) + SO42−(aq)   -0.356 V

Consider the following half-reactions: Ag*(aq) + e¯ → Ag(s) Cu2*(aq) + 2 e¯ → Cu(s) Pb2*(aq) + 2 e¯ → Pb(s) Fe2+(aq) + 2 e→ Fe(s) Al3*(aq) + 3 e¯ E° = +0.80 V E° = +0.34 V E° = -0.13 V E° = -0.44 V → Al(s) E° = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)? O Cu2*(aq) and Fe2*(aq) Fe(s) and Al(s) O Ag*(aq) and Cu2+(ag) O Fe2*(aq) and A13*(aq) O Ag(s) and Cu(s)

A galvanic cell is made of a Ni2+/Ni half cell with [Ni2+] = 6.00 × 10-2 M and an Ag*/Ag half cell with [Ag*] = 4.00 × 10-3 M. Calculate the electromotive force of the cell at 25 °C. The reduction potentials for the two half reactions: Ni2+ (aq) + 2e →Ni(s) Ag*(aq) + e¯ →Ag(s) E° = -0.24 E° = +0.8 O a. 1.14 O b. 0.64 О с. 1.04 O d. 1.06 O e. 0.94

1. Using given standard reduction potentials, calculate the standard potential of a copper−zinc cell: Cu2+(aq) + 2e- → Cu(s) E°= +0.34 V Zn2+(aq) + 2e- → Zn(s) E° = -0.76 V 2. A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V). The button form of this cell is used in watches, hearing aids, and other electronic devices. The half-reactions are: Zn(s) + 2OH- (aq) → Zn(OH)2(s) + 2e- Ag2O(s) + H2O(l) + 2e- → 2Ag(s) + 2OH(aq) (a) Identify the anode and the cathode reactions. (b) What’s the overall reaction in this galvanic cell? 3. Write the cell notation for a galvanic cell with the following half-reactions. (a) Ni(s) → Ni2+(aq) + 2e- Pb2+(aq) + 2e- → Pb(s) (b) Galvanic cell constructed from a hydrogen electrode (cathode) in 1.0 M HCl and a nickel electrode (anode) in 1.0 M NiSO4 solution. The electrodes are connected by a salt bridge. 4. Write the overall cell reaction and draw the fully labelled for the following galvanic cell: Fe(s) Fe2+(aq) Ag+ (aq)…

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Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Zn(3)| Zn*r||Cu*|Cu(e) В © Au(s)|Au|| Mn**|Ma(e) 2+ Co(s)| Co*" Fe* |Fe(e)

Which of the following metals can be oxidized by H+ under standard conditions? Cu, Zn, Ag, Sn     Ag+(aq) + e– → Ag(s) E°  = 0.80 V   Cu2+(aq) + 2e– → Cu(s) E°  = 0.34 V   Cu2+(aq) + e– → Cu+(aq) E°  = 0.15 V   Sn4+(aq) + 2e– → Sn2+(aq) E°  = 0.13 V   Sn2+(aq) + 2e– → Sn(s) E°  = –0.14 V   Zn2+(aq) + 2e– → Zn(s) E°  = –0.76 V

› Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Ni²+] = 0.00100 M and [Au³+] = 0.834 M. Standard reduction potentials can be found in this table. 3 Ni(s) + 2 Au³ +(aq) — 3 Ni² †(aq) + 2 Au(s) E = 1.72 Incorrect V