6.4 Flashcards
(48 cards)
What are two other words for the electrochemical cell
voltaic cell or galvanic cell
What is an electrochemical cell
A portable source of electricity produced by a redox reaction
What is the role of the salt bridge
make both beaker’s contents neutral to prevent electron flow to go backwards.
Oxidation occurs at the _____
anode
Reduction occurs at the _______
cathode
Mass of solid on the anode side will _____ as time passes
diminishes
What is a salt bridge
Porous barrier allowing for ion migration to counterbalance the charge of each solution.
What would happen with no salt bridge to counter-charge the solutions
a charge build-up would occur, the reduction half-cell would become negative and the oxidation half-cell would become positive. Electron flow would stop.
In the salt bridge, anions migrate towards the:
anode
In the salt bridge, cations migrate towards the:
cathode
When is an inverted tube used in the electrode
when the anode or cathode is not a solid, so you can pump gas or liquid into the solution.
How do you calculate the overall voltage of the cell
Add the half-cell potential for the reduction reaction to the inverse of the half-cell potential of the oxidation reaction
The combined voltage will always be ____
positive
What should you never do to the values of the reduction table
multiply them by any coefficient
What is the voltage when equilibrium is reached
0.00 V
in an electrochemical cell, the cathode is the site of
reduction
in an electrochemical cell, the anode is the site of
oxidation
electrons flow from _____ to _____
anode to cathode
In a salt bridge, anions flow to the
anode
in a salt bridge, cations flow to the
cathode
How do you calculate the overall voltage of a cell
add the reduction voltage to the reverse of the oxidation voltage to determine the overal
What is the most common inert
Pt (platinum)
Which substances can’t act as electrodes?
a gas, liquid Hg, Group 1 or 2 metal
in an electrochemical cell, the cathode is the site of
reduction
