Textbook Question
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)
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Ch.19 - Electrochemistry
Chapter 19, Problem 5
Use line notation to represent each electrochemical cell described in Problem 44.
Verified step by step guidance1
Identify the components of the electrochemical cell, including the anode, cathode, and the solutions they are in contact with.
Determine the oxidation and reduction half-reactions occurring at the anode and cathode, respectively.
Write the line notation starting with the anode (where oxidation occurs) on the left and the cathode (where reduction occurs) on the right.
Separate different phases within each half-cell with a single vertical line (|) and separate the anode and cathode compartments with a double vertical line (||), which represents the salt bridge or porous barrier.
Ensure that the line notation reflects the correct order of components: anode material | anode solution || cathode solution | cathode material.
Related Practice
Textbook Question
Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.
b. 2 H+(aq) + Fe(s) → H2(g) + Fe2+(aq)
c. 2 NO3–(aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H2O(l) + 3 Cu2+(aq)
Textbook Question
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. b. KCl(aq) c. CuBr2(aq)
Open Question
The Ksp of Zn(OH)2 is 1.8 * 10^-14. Find Ecell for the half-reaction: Zn(OH)2(s) + 2 e- ⇌ Zn(s) + 2 OH-(aq)
Textbook Question
Balance each redox reaction occurring in acidic aqueous solution. c. BrO3–(aq) + N2H4(g) → Br–(aq) + N2(g)
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Textbook Question
Balance each redox reaction occurring in acidic aqueous solution. a. Zn(s) + Sn2+(aq) → Zn2+(aq) + Sn(s)
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