If we are given a galvanic Cell problem and we are told that the cell consists of one Sn electrode immersed in a 1.00 M solution containing Sn2+ ions, and one Pb electrode immersed in a 1.00 M Pb(NO3)2 solution, how can we determine the cathode/anode? We aren't given any Ecell values.
If the Sn electrode is in Sn2+ solution does that mean it was oxidized?
Why wouldn't the Pb electrode be in an electrolyte solution as well?
If you could please explain I would appreciate it
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Related questions
Which electrochemical reaction is spontaneous in a galvanic cell?
Ni2+(aq) + Cu(s) --> Ni(s) + Cu2+(aq) | ||
Cr3+(aq) + Au(s) --> Cr(s) + Au3+(aq) | ||
Cu2+(aq) + Co2+(aq) --> Cu+(aq) + Co3+(aq) | ||
Cu2+(aq) + Sn(s) --> Cu(s) + Sn2+(aq) |
Which electrochemical reaction is non-spontaneous in an electrolytic cell?
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Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq) | ||||||||||||||||||||||||||||||||||||||
Co2+(aq) + Pb(s) --> Co(s) + Pb2+(aq) | ||||||||||||||||||||||||||||||||||||||
Mn2+(aq) + Ba(s) --> Mn(s) + Ba2+(aq) Which electrochemical reaction is the most spontaneous, generating the highest cell voltage?
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1. 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.
(a) Al and Co(II)
Cathode: ____
Anode: ______
Ecell =
(b) Cd(II) and Ag(I)
cathode: ___
anode: ___
Ecell= ____
(c) Cr(III) and Sc(III)
cathode: ___
Anode:_____
Ecell:____
2. A voltaic cell contains two half-cells. One half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. The second half-cell contains a zinc electrode immersed in a 1.00 M Zn(NO3)2 solution.
Ti3+(aq) + 3 eâ â Ti(s) | Eâ°redâ = â1.370 V |
Zn2+(aq) + 2 eâ â Zn(s) | Eâ°redâ = â0.762 V |
(a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell.
(b) Write the overall balanced equation for the voltaic cell. (Include states-of-matter under the given conditions in your answer.)
3. ÎG° and E° can be said to measure the same thing, and are convertible by the equation
ÎG° = ânFEâ°cellâ
where n is the total number of moles of electrons being transferred, and F is the Faraday constant 9.64853415âââ104 C/mol. The free energy (ÎG°) of a spontaneous reaction is always negative.
For each of the electrochemical cells below, calculate the free energy of the system and state whether the reaction is spontaneous or non-spontaneous as written based on the cathode and anode assignment given. (Use the table of Standard Electrode Potentials.)
(a) The cathode is Zn(II) and the anode is Co(II).
free energy: ____ kJ
spontaneity: _____