Chemistry Definitions
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51 terms
Terms | Definitions |
|---|---|
 formula mass | sum of the atomic masses of all atoms in a compound as represented in a chemical formula; measured in amus |
| empirical formula | chemical formula that gives the simplest whole number ratio of atoms of elements in a compound |
| percent composition | mass of each element in a coup mound relative to the total mass of the compound; found by dividing the mass of the element by the mass of the compound and multiplying the quotient by 100 percent |
| Molar volume of gas @ STP | 22.4 L |
| Carbon 12 | what the scale for atomic mass is based on |
| Determine molar mass | add up the molar masses from the periodic table; measured in grams |
| Solve mass to mass problem | go to grams to moles to moles and back to grams; balance the equation first |
| limiting reactant | a reactant that is completely used up in a chemical reaction and that therefore determines the maximum amount of a product that can be formed |
| stoichiometry | study of quantitative relationships that can be derived from chemical formulas and equations |
| Use Stoichiometry | to find nutritional value, measure concentration of pollution in the atmosphere |
| Hess's La | if a series of reactions are added together the enthalpy change for the net reaction will be the sum of the enthalpy changes for the individual steps |
| endothermic reaction | reaction that absorbs heat, positive, disassociation |
| exothermic reaction | reaction that releases heat, negative, solvation |
| Real gases behave ideally when? | under high temperature and low pressure |
| characteristics of gases | fill up containers completely, can diffuse, are colorless, exert pressure, |
| solvent | substance that does the dissolving in a solution, is larger than the solute |
| solute | substance that is dissolved in a solvent to form a solution |
| making a solution | 1. disassociation- particles separate;needs energy 2. solvation- reaction between solvent and solute;energy is released |
| molality | concentration of a solution determined by the number of moles of a solute over kilogram of solvent |
| Pressure only effects | the solubility of gas in liquids |
| what does adding solute do to the colligative properties? | lowers vapor pressure, raises boiling point, lowers freezing point |
| constant @ equilibrium | the rate of the forward reaction and the reverse reaction/concentrations of reactants and products |
| dynamic equilibrium | reaction recaches equilibrium but reactants are still reacting |
| only factor that will change the value of the equilibrium constant? | temperature |
| large equilibrium constant | the products are favored |
| equilibrium smaller than one | the reactants are favored |
| Arrhenius acid | acid dissociates in water to produce Hydrogen ions |
| Arrhenius base | base dissociates in water to produce hydroxide ions |
| Strong Acids | HCl, HBr, HI, HNO3, H2SO4, HClO4 |
| law of conservation of mass | mass cannot be created nor destroyed in any process |
| specific heat | amount of heat energy required to raise the temperature of 1 gram of a substance by 1 degree celsius |
| heat capacity | amount go heat energy needed to raise the temperature of a given sample of matter by 1 degree Celsius |
| calorimetry purpose | to determine the heat of a reaction |
| Boyle's Law | P1V1=P2V2 |
| Charle's Law | ... |
| Gas volume increases | Pressure decreases |
| temperature increases | volume of gas increases |
| effusion | movement of atoms or molecules through an opening so tiny that they pass through one particle at a time into an evacuated chamber |
| elastic collisions | collide without slowing down or losing energy |
| STP | 1 atm 273 k |
| solution | homogenous mixture of two or more substances in a simple physical state |
| oil and water don't mix because | oil is polar and water is polar, this makes them immiscible |
| factors that effect dissolving rate | surface area, stirring, temperature |
| Raoult's Law | magnitude of vapor pressure reduction is proportional to solute concentration |
| alloy | solid solution in which the atoms of two or more metals are uniformly mixed |
| Q>Eq | shift to the left |
| miscible | ability of a liquid to form a solution with another liquid in all proportions |
| soluble | ability of a substance to dissolve in another substance |
| heterogenous equilibrium | equilibrium condition for a reaction in which all the reactants and products are in two or more different states |
| Le Chatelier's principle | a reversible reaction at equilibrium will shift to offset a stress or change in conditions imposed on the system |
| pH equation | PH=-[concentration] |
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