I need some help with the following two problems:
Determine the cell reaction, the standard cell potential and the half-cell that acts as the cathode for the voltaic cells composed of the following half-cells. Calculate to determine whether the following redox reactions are spontaneous as Written. Show transcribed image text Determine the cell reaction, the standard cell potential and the half-cell that acts as the cathode for the voltaic cells composed of the following half-cells. Calculate to determine whether the following redox reactions are spontaneous as Written.
I need some help with the following two problems:
For unlimited access to Homework Help, a Homework+ subscription is required.
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
Chemistry: The Central Science
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: _____