6. Several cell voltages are given in the following table. The standard reduction potential for the...
please answer the full question. 2. You measured cell potentials (voltages) for reactions of metals and metal ions. We will use the standard date and practice calculating these. Recall: E-Ecathode - Eanode Remember reduction occurs at the cathode; oxidation occurs at the anode For the anode reactions, your reactant will be on the product side of the standard equation, but don't change any sign. The equation does that for you. Cathode Reaction Agt + e → Ag Ecathode Anode Reaction...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
estion 12 of 16 > Consider these two entries from a fictional table of standard reduction potentials. X3+ + 36 - X(s) E° = -2.06 V y3+ +36 Y() E° = -0.15 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?
Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e - X(s) E° = -2.21 V Y3+ + 3e" — Y() E° = -0.42 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? Ecell
Table 1 Cell Type Lithium-iodine Zinc-mercury Operating Cell Potential for Commercial Batteries, E (V) +2.80 +1.35 Table 2 Standard Reduction Potential, E" (V) Half-Reaction Zn(OH).1? +2e → Zn +40H Zn(OH), +2e → Zn +20H HgO + H2O +2e - Hg + 2OH 0, + 2 H2O + 4e 40H - 1.20 |--1.25 +0.10 +0.40 Pacemakers are electronic devices that help regulate the heart rate. Currently, lithium-iodine cells are commonly used to power pacemakers and have replaced zinc-mercury cells. Table 1...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given half-reactions? Reduction Half-Reaction Ered (V) Anode -0.41 Fe2+ (aq) + 2e Fe(s) Cl2 (8) +20 +2 (aq) Cathode 1.36
Consider these two entries from a fictional table of standard reduction potentials. X3+ +36 + X(s) E° = -1.71 V E° = -0.21 V Y3+ + 3e + Y(s) What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? E = +1.78
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
2) On the standard galvanic cell schematic shown below, add labels for: (2 pts) A) Anode B) Cathode C) Salt Bridge D) Show the direction of electron flow through the wire Equations and Constants: AG --FE E-Eº - (RT/nF)InQ R-8.3145 J/mol K F-96485 J/V mole (7 pts) 3) For the galvanic cell represented by Zn(s)Zn²+ (aq)|| Ag (aq)| Ag(s) Voltmeter A) Write the anode half reaction Zn(s) JAg(s) B) Write the cathode half reaction C) Write the net reduction-oxidation reaction...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...