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Stoichiometry and Gas Law Exam
Term 1, Exam 1
43
Chemistry
12th Grade
10/05/2008

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Term
Ammonium
Definition
NH4 +\
Term
Carbonate
Definition
C03 -2\
Term
Sulfate
Definition
SO4 -2\
Term
Phosphate
Definition
PO4 -3\
Term
Nitrate
Definition
NO3 -\
Term
Chlorate
Definition
ClO3 -\
Term
Acetate
Definition
C2H3O2 -\
Term
Hydroxide
Definition
OH -\
Term
Permanganate
Definition
MnO4 -\
Term
Chromate
Definition
CrO4 -2\
Term
An acid with an anion that ends in -ide
Definition
Hyrdo__ic acid (ex: HCl= hydrochloric acid)\
Term
An acid with an anion that ends in -ite
Definition
___ous acid (ex: HNO2=nitrous acid)\
Term
An acid with an anion that ends in -ate
Definition
____ic acid (HC2H3O2=acetic acid)\
Term
Solubility Rule #1
Definition
Salts with the alkali metals and ammonium are soluble\
Term
Solubility Rule #2
Definition
Most chloride, bromide, and iodide salts are soluble except when they contain Ag+, Pb+2, and Hg2 +2.\
Term
Solubility Rule #3
Definition
Most sulfate salts are soluble except for BaSO4, PbSO4, HgSO4, and CaSO4.\
Term
When zero is and isn't a sig fig
Definition
Yes when it is in the middle of a number, no when it's at the beginning of a number, and sometimes when at the end of a number (only with a decimal place or in scientific notation)\
Term
Sig Figs in multiplication and division
Definition
The final answer must have as many sig figs as the number with the lowest amount of sig figs that is not an exact number or conversion\
Term
Sig Figs in addition
Definition
The final answer goes as many digits as the number with the least digits place.\
Term
Volume of a gas at STP
Definition
22.4 L/mol\
Term
Actual yield
Definition
How much the product the reactants actually form\
Term
Theoretical yield
Definition
The amount of product that should be created according to stoichiometry.\
Term
Percent yield
Definition
actual yield divided by theoretical yield\
Term
Empirical formula
Definition
the simplest whole number ratio of atoms in a compound\
Term
Molecular formula
Definition
the exact formula of a molecule, giving the types of atoms and the numbers of each type.\
Term
The five classifications of reactions
Definition
Single replacement, double replacement, combination, decomposition, and combustion.\
Term
Combustion
Definition
With a metal, it makes an ionic compound. If there's carbon, it makes carbon dioxide. If there's hydrogen, it makes water.\
Term
Precipitation reaction
Definition
A double replacement where a cation falls in love with an anion.\
Term
If it's soluble...
Definition
It precipitates out\
Term
Strong acids
Definition
HCl (Hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), H2SO4 (sulfuric acid), H2NO3 (nitric acid), HClO4 (perchloric acid), HClO3 (chloric acid)\
Term
LEO GER
Definition
Less electrons oxidized, greater electrons reduced\
Term
Oxidation state rules
Definition
H is +/-1, O is -2 except when bonded with F, a pure element is 0, sum of all the oxidation sates of a polyatomic ion is equal to the total charge\
Term
Base
Definition
a compound that produces OH- when dissolved in water. It's strong when with Group 1 or lower Group 2 metals\
Term
Spectator ions
Definition
ions not charged in the reaction\
Term
Combined gas law
Definition
(P1V1)/T1 = (P2V2)/T2\
Term
Ideal gas law
Definition
PV=nRT\
Term
R
Definition
R=0.0821 L*atm/mol*K
or 8.31 L*kPa/mol*K\
or 62.4 L*torr/mol*K
Term
Partial pressures
Definition
Pa+Pb+Pc=P total\
Term
Kinetic theory
Definition
The ideal and combined gas laws go under this.\
Term
Assumptions of kinetic theory
Definition
Gas particles are much smaller than the space between them so their volume is negligible, and gas particles are neither attracted nor repelled to one another.\
Term
Non-ideal gases
Definition
Ions are non-ideal, very polar molecules are somewhat non-ideal, and nonpolar molecules are the most ideal. Large molecules are more non-ideal and smaller particles (like noble gases) are more ideal\
Term
Real gas rules
Definition
if particles are attracted to each other, volume smaller than expected. If particles too close together, their mass not negligible, V bigger than expected.\
Term
If a compound has a larger molar mass, it will effuse out...
Definition
Slower\
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