All Flashcards
Label the anode, cathode, and direction of electron flow in a galvanic cell diagram.
Anode: Where oxidation occurs; Cathode: Where reduction occurs; Electron flow: From anode to cathode through the wire.
Label the anode, cathode, and direction of electron flow in an electrolytic cell diagram.
Anode: Where oxidation occurs; Cathode: Where reduction occurs; Electron flow: From the external power source to the cathode, and from the anode back to the power source.
Label the salt bridge in a galvanic cell diagram and explain its function.
Salt bridge: A tube containing an electrolyte (e.g., ) that connects the two half-cells; Function: Maintains charge neutrality by allowing ions to flow between the half-cells.
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.
What are the steps to calculate cell potential (E°) using standard reduction potentials?
- 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?
- 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.