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Write the net redox reaction that occurs in the galvanic cell. Znis) Zn*'(aq) · Pb+2(aq) 1...
Write the net redox reaction that occurs in the following galvanic cell. Ti(s) | Ti- (aq) Se(s) | Se? (aq) 2 Tintaq) + 3 Sets) -- 2 Tirs) + 3 Se raq) Ti(s) • Se(s) - Tu" (aq) - Se="raq) + le 2 T1*(aq) + 3 Se(s) + 1e - 2 TH(s) + 3 Seacaq) Tu(s) Set aq) + 1e - TiB (aq) - Sets) 2 Trs) 3 Seis) -- 2 Tip- aq) + 3 Sep (aq)
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M LiCl electrolyte solution, Pb electrode in a IM Pb(NOsh electrolyte solution. The standard half-cell reduction potentials are given below: Volts 3.05 0.13 Li+(aq) Li(s) 1e + → Write a balanced chemical equation representing the redox chemistry for this galvanic cell. Remember the reaction needs to be spontaneous. a.
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
A galvanic cell is powered by the following redox reaction: MnO 2 (s) + 4 H + (aq) + Zn (s) → Mn + 2 (aq) + 2 H 2 O (l) + Zn + 2 (aq) Cathode half reaction: Anode half reaction: Cell potential under standard conditions:
A galvanic cell has the following reaction. Zn(s) + 2
Fe(aq)
→ 2 Fe(aq)
+ Zn(aq)
E° = 0.72 V
What is the maximum electrical work that can be obtained from this
cell per mole of iron (III) ion?
A galvanic cell is powered by the following redox reaction: O₂(g)+4 H⁺(a q)+2 Zn(s) → 2H₂O(i)+2Zn²⁺(aq)Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions.
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.
A galvanic cell is powered by the following redox reaction: 2 MnO2 (aq) + 16H+ (aq) + 10 Br" (aq) 2 Mn² + (aq) + 8 H2O(1) + 5 Br (1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. 0-0 . 0 Write a balanced equation for the half-reaction that takes place at the cathode. x ? Write a balanced equation for the half-reaction that...
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu? + (aq) + Zn (s) — Cu(s) +Zn² + (aq) Suppose the cell is prepared with 6.36 M Cu? in one half-cell and 3.80 M Zn²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0u ou X 5 ?