What are the steps to calculate cell potential (E°) using standard reduction potentials?
1. Write the half-reactions. 2. Find the standard reduction potentials for each half-reaction. 3. Flip the sign of the oxidation half-reaction. 4. Calculate E°: E° = E°(reduction) + E°(oxidation).
What are the steps for electrolysis of NaCl?
1. Identify the half-reactions (reduction and oxidation). 2. Determine the standard reduction potentials for each half-reaction. 3. Calculate the overall cell potential (E°cell). 4. Apply a voltage greater than or equal to the absolute value of E°cell to drive the non-spontaneous reaction.
What is the effect of a negative E°cell?
The reaction is non-spontaneous and requires an external energy source to proceed (electrolytic cell).
What is the effect of a positive E°cell?
The reaction is spontaneous and can be used to generate electricity (galvanic cell).
What is the effect of multiplying a half-reaction by a coefficient when calculating E°cell?
It has no effect on the standard reduction potential (E°).
What happens if the salt bridge is removed from a galvanic cell?
The cell reaction stops because charge neutrality is not maintained, and ion flow is interrupted.
In an electrolytic cell, what happens if the applied voltage is less than the absolute value of E°cell?
The non-spontaneous reaction will not occur.
What are the key differences between galvanic and electrolytic cells?
Galvanic: Spontaneous, E°cell > 0, generates electricity; Electrolytic: Non-spontaneous, E°cell < 0, requires electrical energy.
Compare and contrast oxidation at the anode in galvanic and electrolytic cells.
Both: Oxidation occurs at the anode. Galvanic: Driven by spontaneous redox reaction. Electrolytic: Driven by external power source.
Compare and contrast reduction at the cathode in galvanic and electrolytic cells.
Both: Reduction occurs at the cathode. Galvanic: Driven by spontaneous redox reaction. Electrolytic: Driven by external power source.
Compare electron flow in galvanic and electrolytic cells.
Galvanic: Electrons flow spontaneously from anode to cathode through an external circuit. Electrolytic: Electrons are forced to flow from anode to cathode by an external power source.
