CHEM 177: EXAM 2
48 Cards in this Set
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nonelectrolyte
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a substance that does not form ions in solutions
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strong electrolyte
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solutes that exist in solutions completely or nearly completely as ions. Essientially all soluble ionic compounds and a few molecular compounds are S.electrolytes
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weak electrolyte
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solutes that exist in solutions mostly in the form of molecules with only a small fraction in the form of ions
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solubility
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the amount of the substance that can be dissolved in a given quantity of solvent at a given temperature
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strong acid
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acids that are strong electrolyts
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Strong Base
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Bases that are strong electrolyts
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Weak Acids/Bases
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Acids and bases that have weak electrolytes (partly ionized)
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precipitate
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an insoluble solid formed by a reaction in solution
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neutralization reaction
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when a solution of an acid and a solution of a base are mixed
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Oxidation
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loss of electrons by a substance
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oxidation number
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each atom in a neutral molecule or a charged species is assigned one. which is the actual charge for a mono atomic ion
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aqueous solution
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solutions in which water is the dissolving medium
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solvent
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the component of the solution that is in the greater quantity
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solute
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the other components
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reduction
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the gain of electrons by a substance
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molarity
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the number of moles of solute per liter of solution
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titration
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the combination of a solution of known concentration with a solution of unknown concentration to determine the unknown concentration or the quantity of solute in the unknown
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equivalence point
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the piont in the titration at which stoichiometrically equivalent quantities of reactants are brought together
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indicator
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used to show the end point of the titration, which coincides closely with the equivalence point
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thermodynamics
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the study of energy and its transformations
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thermochemistry
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the transformation of energy-especially heat-during chemical reactions
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kinetic energy
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energy due to the motion of the object
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potential energy
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energy that an object possesses by virtue of its position relative to other objects
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joule
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The SI unit of energy
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calorie
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another common energy unit
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system
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a specific amount of matter
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surroundings
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everything outside the system
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work
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move
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heat or q
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the energy that is transferred from a hotter object to a colder one
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internal energy or E
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the sum of all the kinetic and potential energies of its component parts
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1st Law of Thermodynamics
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the change in the internal energy of a system is the sum of the heat, transferred into or out of the system and the work done on or by the system
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endothermic
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the system absorbs heat from the surroundings
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exothermic
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the system releases heat to the surroundings
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state function
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the internal energy
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enthalpy (H)
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H=E+PV
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enthalpy of reaction
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The enthalpy of the products minus the enthalpy of the reactants.
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calorimetry
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the amount of heat transferred between the system and the surroundings is measured experimentally by calorimetry
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calorimeter
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measures the temperature change accompanying a process
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heat capacity
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the amount of heat required to raise its temperature by 1K
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molar specific heat
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the heat capacity for one mole of a pure substance
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enthalpy of formation
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the enthalpy change for the reaction in which the substance is formed from its constituent element
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formula weight
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the mass of the collection of atoms represented by a chemical formula
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molecular weight
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the mass of the collection of atoms represented by the chemical formula
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mole
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a collection of avogadros numbers of objects
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stoichiometry
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the relationships among the quantities of reactants and products involved in chemical reactions
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limiting reagent
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the amount of product that can form is limited by the complete consumption of the limiting reactant
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theoretical yield
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the quantity of product that is calculated to form when all of the limiting reagent reacts.
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percent yield
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the ratio of the actual yield of a product to its theoretical yield, multiplied by 100
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CHEM 177: CHAPTER 1