1. Complete the following table comparing galvanic cells and electrolytic cells ! Galvanic Cell pit Spontaneity Electrolytic Cell eht cpontaneous non- cpontaneoms Sign of Standard Cell Potential, Eã Positive hegative Cathode Anode Direction of Electron Movement Direction of lon Movement
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Related questions
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: _____
In thermodynamics, we determine the spontaneity of a reaction by the sign of ÎG. In electrochemistry, spontaneity is determined by the sign of Eâcell. The values of ÎG and Eâcell are related by the following formula: ÎGâ=ânFEâcell where n is the number of moles of electrons transferred and F=96,500J/Vâ mol eâ is the Faraday constant.
Part A The standard reduction potentials of lithium metal and chlorine gas are as follows: Reaction, Reduction potential (V) Li+(aq)+eââLi(s) â3.04
Cl2(g)+2eââ2Clâ(aq) +1.36
In a galvanic cell, the two half-reactions combine to 2Li(s)+Cl2(g)â2Li+(aq)+2Clâ(aq) Calculate the cell potential of this reaction under standard reaction conditions. Express your answer with the appropriate units.
Part B: Calculate the free energy ÎGâ of the reaction. Express your answer with the appropriate units.
Part C:
What can be said about the spontaneity of this reaction?
The reaction is:
a. spontaneous as written. | |
b. spontaneous in the reverse direction. | |
c. at equilibrium. | |
d. nonspontaneous in either direction. |