For Questions 01-02 consider the two standard reduction potentials shown below.
2+ + 2e - → Cu (+0.34V)
+ + e - → ½H 2 (0.00V)
If the two half-cells below were combined in a standard, galvanic cell, what would be the correct chemical equation to represent the spontaneous REDOX process?
If the two half-cells were combined in a galvanic cell, what would be the voltage generated the spontaneous REDOX process?
What is always true of all electrolysis processes?
The metal indium, is known to exist in an oxidation state of +3. What approximate mass of indium (molar mass = 114.82 g) will be produced during the electrolysis of a molten salt that contains In
3+, if a current of 10.0 amps is passed through the electrolyte for a period of 50.0 hours?
The purpose of the salt-bridge in a galvanic cell is
Which combination of values for ΔG°, Keq and E°, is the most likely?
In a simple galvanic cell constructed from the two half-cells shown below,
2+ (aq) + 2e - → Cu (s) +0.34V
Zn 2+ (aq) + 2e - → Zn (s) -0.76 V
Use the following data for Questions 08-10 . The electrolysis of molten sodium chloride yields different products than
the electrolysis of aqueous sodium chloride. The relevant standard electrode potentials
are shown below.
The standard electrode potentials alone, predict that the products from the electrolysis of aqueous sodium chloride should be H
2 gas and O 2 gas, but it is found that in many situations, the actual products are chlorine gas and hydrogen gas. What is the most likely explanation for this observation?
What is the product at the cathode when molten sodium chloride is electrolyzed?
When considering the four reaction reactions listed in the table, it would appear that the reduction of Cl
2 gas to chloride ions is the most reduction likely to occur. Why is Cl 2 gas not reduced at the beginning of the electrolysis of either aqueous, or molten NaCl?