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M: moles of solute dissolved in 1 liter of solution
Molarity
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m: moles of solute per kg of solvent
Molality
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x: mole of solute divided by total moles
mole fraction
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Depend only on the number of solute particles and the identity of the solvent
Ionic materials dissociate
colligative properties
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vapor pressure lowering:
change in P = x (solute) P0(solvent vapor pressure)
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freezing pt. depression:
- change in T = -m(solute)k(fp)
- constant depends on solvent
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boiling pt. elevation
- Change in T = m(solute)k(bp)
- constant depends on solvent
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osmotic pressure:
- II = M (solute) RT
- R is the ideal Gas constant
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accounts for turgor pressure in plants and shap in animal cells
osmotic pressure
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Once seperated from crystal, ions are surrounded by water molecules, this is known as:
solvation
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When the solvent is water, the interactions are also referred to as;
hydration
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The degree of randomness is given by a thermodynamic quantity called:
entropy
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The process where the concentration of solute particles in solution increases, which increases the chances of colliding with the surface of the solid, and the solute particle may become reattached to the solid
Crystallization
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A solution that is in equilibrium with undissolved solute is:
saturated
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The amount of solute needed to form a saturated solution in a given quantity of solvent is known as the:
solubility
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If less solute is dissolved than that needed to form a saturated solution the solution is:
unsaturated
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a solution that contains a greater amount of solute than that needed to form a saturated solution
supersaturated
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The stronger the attractions are btwn solute and solvent molecules:
the greater the solubility
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polar liquids tend to dissolve readily in:
polar solvents
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Nonpolar liquids ten to be insoluble in:
polar liquids
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first basic principle identifying spontaneous processes:
Processes in which the energy content of the system decreases tend to occur spontaneously
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second basic principle identifying spontaneous processes:
Processes occurring at a constant temperature in which the randomness or dispersal in space (entropy) of the system increases tend to occur spontaneously
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formations of solutions is favored by the:
increase in entropy that accompanies mixing
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substances with similar intermolecular attractive forces tend to be:
soluble in one another
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The solubility of the gas increases in direct proportion to:
its partial pressure above the solution
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The solubility of most solid solutes in water increases as:
the temperature of the solution increases
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The solubility of gases in water decreases with:
increasing temperature
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molarity depends on:
the volume of solution
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Molality depends on the :
mass of solvent
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Depend on the collective effect of the number of solute particles
colligative properties
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a substance that has no measurable vapor pressure is:
nonvolatile
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a substance that exhibits a vapor pressure is:
volatile
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When that equilibrium is reached, the pressure exerted by the vapor is called:
The vapor pressure
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The extent to which a nonvolatile solute lowers the vapor pressure is proportuional to its concentration
Raoult's law
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The pressure required to prevent osmosis by pure solvent is the
osmotic pressure
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This forms the dividing line between solutions and heterogeneous mixtures
Colloids
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Scattering of light by colloidal particles
Tyndall effect
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The area of chemistry that is concerned with the speeds, or rates, of reactions is:
Chemical kinetics
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List the 4 factors that affect reaction rates:
- 1. Physical state of the reactants
- 2. Concentrations of the reactants
- 3. Temperature at which the reaction occurs
- 4. The presence of a catalyst
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the change in the concentration of reactants or products per unit of time
raction rate
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Why is it typical for rates to decrease as a reaction proceeds?
because the concentration of reactants decreases
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The exponents m and n in a rate law are called:
reaction orders
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The sum of the orders with respect to each reactant in the rate law
Overall reaction order
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Rate depends on the concentration of a single reactant raised to the first power
A first-order reaction
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Rate depends on the reactant concentration raised to the second power
A second-order reaction
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The time required for the concentration of a reactant to reach one-half of its initial value
Half-life
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How much of the concentration of the reactant is decreased by in a first-order reaction?
1/2 in each of a series of regularly spaced time intervals, namely, t1/2
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based on the kinetic-molecular theory and accounts for reaction rates affected by the concentrations of reactants and the temperature
Collision Model
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The minimum energy required to initiate a chemical reation is called:
activation energy
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The particular arrangement of atoms at the top of the barrier is called
- Activated complex
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- transition state
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The three factors for the Arrhenius equation
- 1. the fraction of molecules possessing an energy of Ea or greater
- 2. The number of collisions occurring per second
- 3. the graction of collisions that have the appropriate orientation
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The process by which a reaction occurs is called the
reaction mechanism
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The number of molecules that participate as reactants in an elementary reation defines its
molecularity
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If a single molecule is involved, the reaction is:
unimolecular
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Elementary reactions ivolving the collision of two reactant molecules are
bimolecular
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Elementary reactions ivolving the simultaneous collision of three molecules are
Termolecular
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If a reaction is an elementary reaction, then its rate law is based directly on its:
molecularity
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rate depends on the concentration
kinetics
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change(reactions)/change(time)
rate average
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change in time
Instaneous Rate
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Why is mixing important?
For rate of reaction to occur to expose surface area for rxn
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What reflects more light?
Fat going into mycelle
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