All Flashcards
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.
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 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.