Consider the reaction 2 Ag(s) + Cu2+ (aq) =2 Ag2+ (aq) + Cu(s). Write the equilibrium...
Identify the complete redox reaction for a CulCu2+||Ag+Ag cell. A. Cu(s) + Ag(s) Cu2+ (aq) + Ag+ (aq) B. Cu(s) + Ag+ (aq) + Cu2+ (aq) + Ag(s) c. Cu(s) + 2 Ag+ (aq) (aq) + 2 Ag(s) D. Cu²+ (aq) + 2 Ag(s) + Cu(s) + 2 Ag+ (aq) → Cu2+
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s) Eo= 0.8V If you increase the concentration of Cu2+(aq), which of the following would be true about the cell potential E? It would remain constant It would increase It would decrease This cannot be determined
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standard potential for the cell reaction for 2 Ag + H2 (g)-2 Ag+2H +0.80 V b. a. +0.40 V +0.12 V d. c. -0.12 v none of these e. 40. Given: Fe (s) + 2 Ag' (aq) Fe (ag)+ 2 Ag (s) with E ell -1.24 V What is the...
A voltaic cell set up utilizing the reaction Cu(s) + 2 Ag+ (aq) → Cu2+ (aq) + 2 Ag (s) has a cell potential of 0.45 V at 298 K. Describe how the potential of the cell will change as the cell is discharged. At what point does the cell potential reach a constant value? Explain your answer
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai (aq)3eAl (s) Eo0.7996 V E0.342 V Eo-1.6632 V i. Which pair of half reactions would make the battery with the largest E cell? i. Identify the cathode and the anode for this battery, and calculate the value of E cell. i. Write the overall redox reaction that would take place in the battery above.
3. Consider the following redox reaction: Zn Zn (s) +Cu2 (aq) (aq)+ Cu (s) 3.a. (10 p) Indicate the line diagram of the galvanic cell that uses the spontaneous redox reaction shown above. 3.b. (5 p) Write the reduction reaction corresponding to each half-cell. 3.c (5p)Calculate the equilibrium constant of the reaction K using the Nemst equation. Refer to Appendix H in the textbook to find the E values.
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +e → Ag(s) 0.799V Cu2+(aq) + 2e → Cu(s) 0.337V Mg2+(aq) + 2e —— Mg(s) -2.370V The strongest oxidizing agent is: enter symbol The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will Mg(s) oxidize Ag(s) to Ag+(aq)? V Which species can be oxidized by Cu2+(aq)? If none enter none. Consider the following half-reactions: Half-reaction E° (V) 2Br (aq) 1.080V Br2(1) + 2e — Ni2+(aq) +...
Consider the following reaction: 2 Ag+(aq) + Cu(s)->2 Ag(s) + Cu2+(aq) Ecell^o = +0.46V Suppose an external power source is applied with a current of 1.50 A such that the reaction is reversed and electrolysis occurs. (a) If the current is applied for 2.00 hours, how many grams of Cu(s) could be recovered? What is the minimum mass of the silver electrode required to recover this mass of copper? (b) What is the minimum amount of work that must be...