Tuesday, February 8, 2011
Tues-Day 1
Physics - we did all of Circuits 5 on parallel circuits, and then we set up series circuits, and determined that each resistor in the circuit obeyed Ohm's Law.
AP Chem - started with a review of equilibrium constant expressions in terms of concentrations or in terms of partial pressures of gases (if any).
Large K values indicate that the PRODUCTS are "favored" at EQUILIBRIUM.
Small K values indicate that the REACTANTS are "favored" at EQUILIBRIUM.
We saw that, when the equation stoichiometric coefficients are multiplied by a given factor, x, that the resulting equilibrium constant is taken to that EXPONENT, x.
When the products and reactants are written in reverse, the resulting K is the RECIPROCAL of the original K.
We also showed how to combine the equilibrium constants from several reactions; addition of reactions causes the MULTIPLICATION of the respective equilibrium constants to get the NET equilibrium constant for the overall reaction.
We discussed "REACTION QUOTIENT" which is the same EXPRESSION as K , HOWEVER, the quantities plugged in to the expression are NOT the equilibrium concentrations! The quantities plugged into the expression are the INITIAL concentrations.
By comparing K with Q, one can determine whether the reaction will proceed towards either forming more reactants or more products as equilibrium is approached.
AP Chem - started with a review of equilibrium constant expressions in terms of concentrations or in terms of partial pressures of gases (if any).
Large K values indicate that the PRODUCTS are "favored" at EQUILIBRIUM.
Small K values indicate that the REACTANTS are "favored" at EQUILIBRIUM.
We saw that, when the equation stoichiometric coefficients are multiplied by a given factor, x, that the resulting equilibrium constant is taken to that EXPONENT, x.
When the products and reactants are written in reverse, the resulting K is the RECIPROCAL of the original K.
We also showed how to combine the equilibrium constants from several reactions; addition of reactions causes the MULTIPLICATION of the respective equilibrium constants to get the NET equilibrium constant for the overall reaction.
We discussed "REACTION QUOTIENT" which is the same EXPRESSION as K , HOWEVER, the quantities plugged in to the expression are NOT the equilibrium concentrations! The quantities plugged into the expression are the INITIAL concentrations.
By comparing K with Q, one can determine whether the reaction will proceed towards either forming more reactants or more products as equilibrium is approached.
# posted by C @ 11:18 PM 
