9B Galvanic Flashcards
How do you balance Redox (basic) in steps
- Use the Half reaction for acidic solution to balance as if H+ ions were present
- Add OH- ions needed to balance the H+ ions in last step
- Form H2O on sides containing both and cancel water molecules on both side
- Check to see if Balanced equation
Anode
Oxidation (Electrons flow away) at the Negative end
Cathode
Reduction (Electrons flow in) at the Positive end
Salt Bridge
Tube containing the electrolyte providing contact between two solutions
How to express work with a moving charge
W=-qdE
Q=charge (V), dE=potential difference (-w elec)
What is free energy
The energy available to do work
What is dE=E cell ‘s meaning
The difference in elecetrial potential between the anode and cathode in an electrochemical cell
E cell is commonly referred to as
- Cell voltage
- Electromotive force (emf)
- Cell potential
Standard Reduction Potential (E^0)
The potential associated with a reduction reaction at an electrode when all solutes are 1 M and all gases are at 1 atm
Standard hydrogen electrode
Accepted reference point (E=0 V)
Why is the SHE important
All standard reduction potentials are measured relative to the SHE (0 V)
Electrode potentials are always measured ____ to each other
Relative
How do you know if something is a Cathode by observing a Galvanic cell
Electrons flow towards it
Reduction (Oxidizing agent) and standard reduction potential (E) relationship
The more positive E, more like to be reduced
What effect does changing the stoicheometric coefficients have on E^0
No effect
