april 20-25, 2015
molarity (m)
THE NUMBER OF MOLES OF SOLUTE DISSOLVED PER LITER OF SOLUTION
m=MOLES SOLUTE
LITERS SOLUTION
dilution FORMULA FOR MOLARITY
m1 X v1 = m2 X v2
April 13-17, 2015
SOLUTION
a homogeneous mixture.
SOLUTE
the dissolved particles in a solution
SOLVENT
the liquid in which a solute is dissolved to form a solution.
SOLUBILITY
the amount of substance that dissolves in a given quantity of solvent at a specific temperature and pressure to produce a saturated solution
SOLUBLE
able to be dissolved
INSOLUBLE
not able to be dissolved
MISCIBLE
liquids that will dissolve in each other
IMMISCIBLE
liquids that will not dissolve in each other
DISSOCIATION
The process by which the action of a solvent causes a molecule to split into simpler groups of atoms, or ions.
FACTORS THAT AFFECT SOLUBILITY
AGITATION
creates more collisions between solute and solvent
SURFACE AREA
more surface area allows for more collisions
TEMPERATURE
more solid solute will dissolve at a higher temperature. Increased temperature increases the speed of the particles and increases the collisions.
SATURATED SOLUTION
a solution containing the maximum amount of dissolved solute at a given temperature and pressure.
UNSATURATED SOLUTION
a solution containing less then the maximum amount of dissolved solute at a given temperature and pressure.
SUPERSATURATED SOLUTION
a solution that contains more solute then it can theoretically hold at a given temperature and pressure
CONCENTRATION
a measurement of the amount of solute that is dissolved in a given quantity of solvent
MOLARITY (m)
THE NUMBER OF MOLES OF SOLUTE DISSOLVED PER LITER OF SOLUTION
m=MOLES SOLUTE
LITERS SOLUTION
DILUTION FORMULA FOR MOLARITY
m1 X v1 = m2 X v2
SOLUBILITY CURVE
A graph showing the concentration of a substance in a solvent as a function of temperature.
April 29, 2014
students made molar solutions in the lab
Molar dilutions
M1 x V1 = M2 x v2
Factors that Affect Solubility
Agitation
creates more collisions between solute and solvent
Surface area
more surface area allows for more collisions
Temperature
more solid solute will dissolve at a higher temperature. Increased temperature increases the speed of the particles and increases the collisions.
Henry's Law
at a given temperature, the solubility(s) of a gas in a liquid is directly proportional to the pressure(P) above the liquid.
S1 = S2
P1 P2
Colligative properties
physical properties of solutions that depend only on the number of dissolved particles.
Vapor pressure lowering
adding a solute to a solvent lowers the solvents vapor pressure.
Boiling point elevation
adding a solute to a solvent will raise the boiling point
Freezing point depression
adding a solute to a solvent will decrease the freezing point
April 23, 2014
Solution
a homogeneous mixture.
solute
the dissolved particles in a solution
solvent
the liquid in which a solute is dissolved to form a solution.
solubility
the amount of substance that dissolves in a given quantity of solvent at a specific temperature and pressure to produce a saturated solution
soluble
able to be dissolved
insoluble
not able to be dissolved
miscible
liquids that will dissolve in each other
immiscible
liquids that will not dissolve in each other
saturated solution
a solution containing the maximum amount of dissolved solute at a given temperature and pressure.
unsaturated solution
a solution containing less then the maximum amount of dissolved solute at a given temperature and pressure.
supersaturated solution
a solution that contains more solute then it can theoretically hold at a given temperature and pressure
concentration
a measurement of the amount of solute that is dissolved in a given quantity of solvent
percent by mass
% mass = mass solute x 100
mass solution
percent volume
% volume = volume solute x 100
volume solution
molarity (m)
THE NUMBER OF MOLES OF SOLUTE DISSOLVED PER LITER OF SOLUTION
m=MOLES SOLUTE
LITERS SOLUTION
dilution FORMULA FOR MOLARITY
m1 X v1 = m2 X v2
April 11,2014
students took quarterly
April 1 , 2014
Dalton's Law of Partial Pressure
at constant volume and temperature the total pressure of a mixture of gases is a sum of the partial pressure of each gas.
Pt = P1 + p2 + p3 ......
Graham's Law of Effusion
the rate of effusion of a gas is inversely proportional to the square root of it's molar mass
April 29, 2013
Honors
reversible reaction
a chemical reaction that can occur in both the forward and reverse directions
Chemical equilibrium
state at which the forward reaction is equal to the reverse reaction
Equilibrium position
The concentrations of the reactants and products at equilibrium
At a given temperature a chemical system will reach a state in which a specific ratio of the reactants and products is a constant.
Equilibrium constant
The ratio of the product concentration to the reactant concentration raised to the power of the moles of the substance from a balanced chemcial equation.
Factors that affect chemical equilibrium
Le Chatelier's Principle
If a stess is applied to a system at equilibrium, the system shifts in the direction that relieves the stress
Changes in concentration
a) Adding reactant causes the reaction to shift to the right
b) Adding product causes the reaction to shift to the left
c) Removing reactant causes the reaction to shift to the left
d) Removing product causes the reaction to shift to the right
Changes in pressure (only affects gaseous reactions)
a) increases the pressure causes the raction to shift in the direction of less moles.
b) decreasing the pressure causes the reaction to shift in the direction of more moles.
Changes in temperature
a) increasing the temperature of an exothermic reaction causes the reaction to shift to the left
b) increasing the temperature of an endothermic reaction causes the reaction to shift to the right
c) decreasing the temperature of an exothermic reaction causes the reaction to shift to the right
d) decreasing the temperature of an endothermic reaction causes the reaction to shift to the left
Students worked on a LeChatier lab
le_chatier_lab.pdf | |
File Size: | 95 kb |
File Type: |
April 25, 2013
Honors
reversible reaction
a chemical reaction that can occur in both the forward and reverse directions
Chemical equilibrium
state at which the forward reaction is equal to the reverse reaction
Equilibrium postiion
The concentrations of the reactants and products at equilibrium
At a given temperature a chemical system will reach a state in which a specific ratio of the reactants and products is a constant.
Equilibrium constant
The ratio of the product concentration to the reactant concentration raised to the power of the moles of the substance from a balanced chemcial equation.
Factors that affect chemical equilibrium
Le Chatelier's Principle
If a stess is applied to a system at equilibrium, the system shifts in the direction that relieves the stress
Changes in concentration
a) Adding reactant causes the reaction to shift to the right
b) Adding product causes the reaction to shift to the left
c) Removing reactant causes the reaction to shift to the left
d) Removing product causes the reaction to shift to the right
Changes in pressure (only affects gaseous reactions)
a) increases the pressure causes the raction to shift in the direction of less moles.
b) decreasing the pressure causes the reaction to shift in the direction of more moles.
Changes in temperature
a) increasing the temperature of an exothermic reaction causes the reaction to shift to the left
b) increasing the temperature of an endothermic reaction causes the reaction to shift to the right
c) decreasing the temperature of an exothermic reaction causes the reaction to shift to the right
d) decreasing the temperature of an endothermic reaction causes the reaction to shift to the left
April 23, 2013
Honors
reversible reaction
a chemical reaction that can occur in both the forward and reverse directions
Chemical equilibrium
state at which the forward reaction is equal to the reverse reaction
Equilibrium postiion
The concentrations of the reactants and products at equilibrium
At a given temperature a chemical system will reach a state in which a specific ratio of the reactants and products is a constant.
Equilibrium constant
The ratio of the product concentration to the reactant concentration raised to the power of the moles of the substance from a balanced chemcial equation.
Factors that affect chemical equilibrium
Le Chatelier's Principle
If a stess is applied to a system at equilibrium, the system shifts in the direction that relieves the stress
Changes in concentration
a) Adding reactant causes the reaction to shift to the right
b) Adding product causes the reaction to shift to the left
c) Removing reactant causes the reaction to shift to the left
d) Removing product causes the reaction to shift to the right
Changes in pressure (only affects gaseous reactions)
a) increases the pressure causes the raction to shift in the direction of less moles.
b) decreasing the pressure causes the reaction to shift in the direction of more moles.
Changes in temperature
a) increasing the temperature of an exothermic reaction causes the reaction to shift to the left
b) increasing the temperature of an endothermic reaction causes the reaction to shift to the right
c) decreasing the temperature of an exothermic reaction causes the reaction to shift to the right
d) decreasing the temperature of an endothermic reaction causes the reaction to shift to the left
April 23, 2013
Honors
reversible reaction
a chemical reaction that can occur in both the forward and reverse directions
Chemical equilibrium
state at which the forward reaction is equal to the reverse reaction
Equilibrium postiion
The concentrations of the reactants and products at equilibrium
At a given temperature a chemical system will reach a state in which a specific ratio of the reactants and products is a constant.
Equilibrium constant
The ratio of the product concentration to the reactant concentration raised to the power of the moles of the substance from a balanced chemcial equation.
April 19,2013
Honors
Heating and cooling curve
A graph of temperature vs time that show the changes of state of a substance
Phase Diagram
A graph of pressure vs temperature that shows the phase of a substance at different pressures and temperatures
Triple Point
conditions of pressure and temperature in which all three phases coexist
Spontaneous process
Any chemical or physical process that once begun, occurs with on outside intervention
Entropy
the measure of disorder of a system
Rate of reaction
the change in concentration of reaction or product per unit time
Collision Theory
In order for atoms, ions or molecules to react they must:
a) collide
b) collide with the proper orientation
c) collide with the minimun activation energy
Factors that affect reaction rate
a) nature of the reactants
b) concentration
c) surface area
d) temperature
e) catalyst or inhibitor
April 17,2013
Honors
catalyst
a substance that accelerates the rate of a chemical reaction by lowering the activation energy of the reaction. A catalyst does not change the enthalpy of reaction.
Spontaneous process
Any chemical or physical process that once begun, occurs with on outside intervention
Entropy
the measure of disorder of a system
Heat (Enthalpy) of combustion
the heat (enthalpy) change for the complete burning of 1 mole of a substance.
Students worked on the heat of combustion worksheet. Download below.
April 15,2013
Honors
Thermochemistry
The study of heat changes that accompany chemical reactions and phase changes
Universe = system + surrounds
exothermic
a reaction or process in which heat is released by the system
endothermic
a reaction or process in which heat is absorbed by the system
Enthalpy (H)
heat content of a system at constant pressure
Enthalpy (Heat)of reaction
The change in enthalpy (heat)for a reaction
^Hrxn = Hp - Hr
^H is - for an exothermic reaction and + for an endothermic reaction.
Thermochemical equation
A balanced chemical equation that includes the energy change and the physical states of all the reactants and products
Students worked on a " energy diagram for a reaction" worksheet that can be downloaded below.
heat_of_reaction_ws.pdf | |
File Size: | 98 kb |
File Type: |
Enthalpy (heat) of combustion
of a substance is the enthalpy (heat) change for the complete burning of one mole of a substance.
Students worked on the heat of reaction worksheet that can be downloaded below
energy_diagram_for_reaction_ws.pdf | |
File Size: | 52 kb |
File Type: |