If you look at the table, All except Fe are below Sn, so only Fe can reduce Sn from its solution. Which of the following is the correct cell notation for this reaction? O Fel Fe*2 || Sn+21 Sn O Sn I Sn*2 || Fe+21 Fe O Cell notation can not be written for this reaction O I don't know what reduction means

Which of the following is the correct shorthand notation for the overall cell reaction given below.        Mg(s)  +  Cu2+(aq)  →  Mg2+(aq)  +  Cu(s)   Select one: a. Mg(s) | Mg2+(aq) || Cu2+(aq) | Cu(s) b. Cu(s) | Mg2+(aq) || Cu2+(aq) | Mg(s) c. Mg(s) | Cu2+(aq) || Mg2+(aq) | Cu(s) d. Cu(s) | Cu2+(aq) || Mg2+(aq) | Mg(s)

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Al(s) + 312 (s) → 2Al3+ (aq) + 6I¯ (aq) 3+ The emf generated by the cell when [Al] = 3.0 · 10- M and [I¯] = 0.50 M is %3D V. 2.23 2.27 2.20 2.13 2.34

What is AG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°cell = 0.317 V?

Consider the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) What is the half-cell reaction for reduction? Multiple Choice О Fe(s) -> Fe2+(aq) + 2 e- Cu2+(aq) + 2 e-→ Cu(s) О Cu(s) → Cu2+(aq) + 2e- Fe(s) + 2 e-→ Fe2(aq)

4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…

Given the cell notation: Snis) | Sn2* (aq) || Fe3* (aq) | Fe(s) The oxidation number of Sn 1 Select ] V, Sn is I Select ] Electrons are transferred from [Select] v to I Select )

For a voltaic cell based on the reaction below, what reaction happens at the cathode?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g)   a. Zn(s)→Zn2+(aq)+2e-   b. 2H+(aq)+2e-→H2(g)   c. Zn2+(aq)+2e-→Zn(s)   c. H2(g)→2H+(aq)+2e-

Find K for the following reaction at at 25°C. E cell = -0.10 V Cd²+ (aq) + Fe(s) Cd(s) + Fe2+ (aq) 4.2 x 10-4 O 1.2 x 10-5 1.2 x 105 4.2 x 1010