Term
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Definition
process in which soluble ionic reactants yeild an insoluble solid product that falls out of the solution, there by removing some of the dissolved ions
-anions and ions switch partners
-(aq)+(aq)--->(aq)+(s) |
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Term
| oxidation-reduction (redox) |
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Definition
| one or more electrons are transferred between partners |
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Term
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Definition
-ionic substances that dissolve in water producing solutions of ions
-when ionic substance dissolves in water the solution contains seperate cation and anions surrounds by water because the presents of charged ions the ionic solution conducts electricity
-a solution that completely dissociates into ions is a stronger electrolyte than one that only partially dissociates into ions |
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Term
| to predict a precipitation reaction |
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Definition
you must know the solubility
-if a substance has low solubility in water it's likely to precipitate |
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Term
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Definition
| solubility is most favorible when there is a strong attraction of solute particals to solvent particals
1. a compound is likely solube if it contains the cations:
- group 1A: Li+,Na+,Rb+,Cs+
2.a compound is likely solube if it contains the anions:
-except if paired with Ag+,Hg2+,Pb2+
-except if paired with Ba2+,Hg2+,Pb2+ sulfates |
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Term
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Definition
| substance that dissociates in water to give H+ |
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Term
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Definition
| substances that dissociate in water to give HO- |
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Term
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Definition
acids that contain oxygen and hydrogen and another element |
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Term
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Definition
| when acids and bases are mixed right both acidic and basic properties dissappear because of neutralization reaction and produce water and salt |
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Term
| acid base neutralization reactions |
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Definition
-always produce salt
-water is only produced in neutralization reactions that involve a strong base
if the carbonate ion is involved the reaction may produce carbon gas |
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Term
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Definition
| (when water is the solvent) when an ionic solid dissolves in a liquid the ions dissociate and become surroundedd by solvent molecules |
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Term
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Definition
acids that dissociate to a large extent and are strong electrolytes
-HClO4,H2SO4,HBr,HCl,HNO3 |
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Term
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Definition
acid that dissociate only and small percent and are weak electrolytes
-H3PO4,HF,CH3CO2H |
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Term
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Definition
most are metal hydroxides and are strong electrolytes
-NAOH,KOH,Ba(OH)2,Ca(OH)2 |
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Term
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Definition
| the man who discovered the essential nature of acids through solution conductivity |
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Term
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Definition
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Term
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Definition
| the names of oxoacids are related to the names of corresponding oxoanions, with the -ite or ate ending of the anion replaced by -ous acid or -ic acid and the acid w/ more oxygens has an ic ending |
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Term
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Definition
| capacity to supply heat or do work, either kinetic or potential |
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Term
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Definition
(Ek) energy of motion
Ek=1/2mv2
m=mass
v=velocity in meters per second |
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Term
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Definition
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Term
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Definition
| the measure of kinetic energy of molecular motion |
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Term
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Definition
| the energy transferred from one object to another is the result of temperature difference between them |
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Term
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Definition
the distance moved times the force that opposes the motion
-w=Fxd |
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Term
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Definition
-sum of all kinetic and potential energies for every molecule or ion in the system -any energy that flows from the system to the surroundings has a negative sign because the system has lost it (Efinal is smaller than Einitial)
-any energy that flows to the system from the surroundings has a positive sign because the system has gained it |
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Term
| the 1st law of thermodynamics |
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Definition
-the total system internal energy of an isolated system is constant
-energy cannot be created or destroyed, it can only be converted from one form to another
- the energy of the universe stays constant |
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Term
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Definition
a function or property depends only on the present state or condition of the system, not the pat it used to arrive at that state
- pressure, volume, and temperature are all state functions but work and heat are not
-reveribile |
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Term
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Definition
the amount of heat required to raise the temperature of an object or substance by a given amount
-C=q/ΔT
-the greater the heat capcity the greater the amount of heat needed to produce a given temperature change |
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Term
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Definition
- ΔE=q+w=q-PΔV, q= transferred heat
- if a system does work on its surroundings (E flows out of the system) w is negative, if the surroundings do work of the system (E flows into the system) w is positive where as -q has a positive sign if the system gains heat and a negative sign if the system loses heat
- q=ΔE+PΔV
- qv=ΔE at constant volume (ΔV=0)
- ΔE=(KJ/°C)(°C)
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Term
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Definition
| if the products of a reaction have less enthalpy than the reactants then the heat has flowed out of the system to the surroundings and ΔH has a positive sign |
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Term
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Definition
- thought to be decaded remains of acient marine organisms
- must be seperated into fractions (by boiling) in order to be used effeciently
- commercial uses include gasoline and kerosene all w/ different numbers of carbon atoms
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Term
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Definition
| fossil fuel that was formed from the remains of plants that were buried and exposed to high pressure and heat over time |
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Term
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Definition
| fossil fuel that was formed by primarily methane |
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Term
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Definition
| if no volume changes occurs and no work is done then ΔH and ΔE are the same |
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Term
| heat of combustion (combustion enthalpy) |
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Definition
| the standard enthalpy for the reaction of 1 mole of substance with oxygen |
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Term
| standard heat of formation |
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Definition
the enthalpy change Δ°Hf for the formation of 1 mole of a substance in its standard stae from it constituent elements in their standard states
- ΔHreaction=Δ°Hf(products)-Δ°Hf(reactants)
-KJ=(a mols)(A KJ/mol)+(b mols)(B KJ/mol)-(c mols)(C KJ/mol) |
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Term
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Definition
H2(g)+1/2O2(g)--->H2O(l)
CH4(g)+2O2(g)--->CO2(g)+2H2O(l) |
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Term
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Definition
| the amount of enery that must be supplied to break a chemical bond in an isolated molecule in the gaseous state and is thus the amount of energy released when the bond forms |
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Term
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Definition
| the overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps in the reaction |
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Term
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Definition
ΔH=ΔE+PΔV
enthaply change:
(specific heat•added mass•temperature change)÷(moles of sustance) |
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Term
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Definition
have values that do not depend on sample amount
-temperature, melting point |
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Term
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Definition
have values that do depend on the amount of sample
-length, volume |
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Term
| calculating the amount of heat released |
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Definition
1. convert grams to moles
-grams • 1mole/amu
2. multiply answer by Δ°H given over the number of moles in the problem
-x moles • KJ/x moles in the equation= KJ |
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