explain chemical equilibrium as a reaction mixture whose composition is unchanging in time, and relate this to the kinetic picture of equal rates of formation and decomposition of reactants and products
define the equilibrium constant, and write it down for an arbitrary gas phase reaction
calculate the value of the equilibrium constant for a reverse reaction from its value for a forward reaction, and if the stoichiometry is changed
calculate the equilibrium constant for a reaction obtained by combining two other reactions
calculate equilibrium compositions from starting compositions and the equilibrium constant for a simple gas phase reaction
calculate the equilibrium composition for a chemical reaction from its equilibrium constant and mass balance information
use appropriate aproximations for simplifying such calculations
define the reaction quotient and use it to predict the direction of change in a reaction as it approaches equilibrium, or if it is perturbed from equilibrium.
use the enthalpy of reaction to predict how the equilibrium constant changes with temperature
explain that catalysts change the pathway and rate of reaction but not the position of equilibrium
explain that entropy depends on concentration, but enthalpy can be treated as independent of concentration
explain the reasons for the conditions used in the Haber Process, and apply the same reasoning to the optimization of other chemical processes, such as smelting
Identify oxidation and reduction half-reactions, and combine them into a balanced redox reaction
explain how a Galvanic cell is constructed to draw a current from a redox reaction
use the activity series to decide which element or compound is the stronger oxidant
calculate the (standard) cell potential and determine the spontaneous direction of a redox reaction under standard conditions
calculate the cell potential for standard and non-standard conditions from the half-cell reactions, and determine the spontaneous direction of a redox reaction
calculate equilibrium constants from standard cell potentials and vice versa
combine reaction quotient and cell potential information to solve for unknown concentrations both at equilibrium and away from equilibrium
identify the key design features of an electrochemical sensor, and calculate an unknown concentration for appropriate electrochemical data
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