Chem II: Final Flashcards
exploits the effect of concentration changes on cel potential
a concentration cell
as long as the concentrations of the solutions are different, the cell potential is — and the cell can do work
greater than 0
the cell is no longer able to do work when —
the concentrations are equal
monitors the [H+] of the solution relative to its own fixed internal [H+]
glass electrode
uses electrical energy from an external energy from an external source to drive a nonspontaneous redox reaction
electrolytic cell
electrons flow from — to —
cathode to anode
the spitting of a substance by the input of electrical energy
electrolysis
the amount of substance produced at each electrode is directly proportional to the quantity of charge flowing through the cell
Faraday’s law of electrolysis
a battery consists of —
self-contained voltaic cells arranged in series, so their individual voltages are added.
— cannot be recharged. the battery is dead when it reaches equilibrium
primary battery
is rechargeable. electrical energy is supplied to reverse the cell reaction and form more reactant
secondary battery
in a — cell, reactants enter the cell and products leave, generating electricity through controlled combustion
fuel cell or flow cell
the process whereby metals are deteriorated via an electrochemical process
corrosion
the time required for the concentration of a reactant to decrease to half of its initial concentration
half life
focuses on the importance of effective molecular collisions
collision theory
focuses on the high energy species (called the transition state) that forms during effective molecular collisions
transition state theory
affects the number of collisions
concentration and temperature
all reactions require a minimum amount of energy to produce effective collisions. This is the —
activation energy
the lower the activation energy, the — the rate
faster
an effective collision between particles leads to the formation of a — or —
transition state or activated complex
the sequence of a single reaction steps that make up the overall equation
mechanism
the individual steps of the reaction are called — bc each one describes a —
elementary steps
single molecular event
formed and then consumed during the course of the reaction; not as stable as reactants or products; more stable than transition states; super reactive
intermediates
the slowest step in a reaction is the — step
rate-limiting step
a mechanism is a —
hypothesis
speeds up the rate of reactions by lowering the total activation energy
catalyst
higher bond order = — activation energy
higher
