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47 Cards in this Set
- Front
- Back
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Avagadro's number |
How many particles are in a mole 6.02x10^23 |
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Mole |
SI Unit for measuring the amount substance of an object |
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Molar Mass |
The mass in grams of one mole of any substance |
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Empirical Formula |
The smallest whole number mole ratio of the elements |
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Molecular Formula |
The actual number of atoms in an element |
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Percent Composition |
Percent by mass of each element in a compound |
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Stoichiometry |
Study of quantitative relationships between amounts of reactants and products |
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Mole Ratio |
Ratio between number of moles of any two substances |
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Limiting Reactant |
Reactant that limits the equation |
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Excess reactant |
Leftover reactant |
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Theoretical yield |
Maximum amount of product that can be produced from a reaction |
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Actual yield |
Amount actually produced |
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Percent yield |
Actual yield/theoretical yield • 100 |
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Kinetic theory |
Gases don't attract or repel, smaller than the distance between them, constant random motion, no kinetic energy is lost when they collide, same kinetic energy at a given temperature |
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Boyle's Law |
Volume at a constant temperature varies with pressure-- P1(V1)=P2(V2) |
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Charle's Law |
Volume is directly promotional to its Kelvin temperature at constant pressure-- V1/T1=V2/T2 |
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Gay-Lussac's Law |
Pressure is directly proportional to temperature at constant pressure--P1/T1=P2/T2 |
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Ideal Gas Law |
PV=nRT |
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Solution |
Homogeneous mixture containing 2+ substance |
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Solute |
Substance that dissolves |
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Soluble |
When a substance is able to dissolve in a solute |
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Insoluble |
Doesn't dissolve in water |
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Combined Gas Law |
P1(V1)/T1=P2(V2)/T2 |
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Avogadro's principle |
Volumes of gas at the same temperature and pressure contain an equal number of particles |
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Immiscible |
2 liquids the are insoluble to each other |
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Miscible |
2 liquids that are soluble |
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Solvation |
Process of surrounding solute particles with solvent particles to form a solution |
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Solubility |
Maximum amount of solute that will dissolve in an amount of solvent at a specified temperature and pressure |
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Saturated solution |
Contains the maximum amount of the dissolved solute for an amount of solvent at a specified temperature and pressure |
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Unsaturated solution |
Contains less dissolved solute for a given temperature and pressure than a saturated solution |
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Henry's Law |
S1/P1=S2/P2 |
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Concentration |
How much solute is dissolved in a specific amount of solvent of solution |
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Molarity |
Number of moles dissolved per liter of solution (moles of solute)/(liters of solution) |
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Stock solution |
Highly concentrated solution provided for experimentation |
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Molality |
(Moles solute)/(kilograms of solvent) |
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Mole fraction |
Moles of solute to total moles of solute and solvent (solution) |
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Colligative properties |
Physical properties of solutions |
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Suspension |
Mixture containing particles that settle out of left undisturbed |
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Colloid |
Heterogeneous mixture of intermediate size particles |
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Brownian motion |
Erratic movement of colloid particles |
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Tyndall effect |
Phenomenon of colloids that allows them to scatter light |
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Chemical equilibrium |
State in which all are balanced |
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Law of chemical equilibrium |
At a given temperature constant values |
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Homogenous equilibrium |
All reactants in the same physical state |
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Heterogeneous equilibrium |
Present in more than one state |
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Properties of acids |
H+, sour, sharp, tart, turns pink |
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Properties of bases |
OH-, bitter, slippery, turns blue |
