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61 Cards in this Set
- Front
- Back
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CHAPTER 6
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Formula or molecular mass |
atomic mass in the chemical formula |
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molecular Mass |
mass in AMU for a molecule from nonmetal elements forming covalent Bonds |
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Molecule |
is a covalent compounds smallest unit, mades of nonmetals in covalent bonds |
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Formula Mass |
mass in AMU for a formula unit or for all compounds |
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Formula Unit |
is the smallest whole number ratio of an ionic compound with metallic and nonmetallic elements |
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Mass of hydrogen atom |
1.673 x 10^-24 g |
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Mole |
a unit for counting chemist require for conting which can express large numbers of atoms using simple numbers |
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Avagardo's Number * NOTE: 1 mole of any elements is eqivalent to ??? |
6.0221 x 10^23 |
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Atoms or Molecules ----> Moles Moles----> Atoms or Molecules |
Atoms or Molecules/ Avogadro's # = MOLES Moles x Avogadro's # = ATOMS or MOLECULES |
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Moles ----> Mass(grams) Mass(grams)---->Moles |
Moles x Molar Mass= MASS Mass(grams)/Molar Mass= MOLES |
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Mass(grams) ----> Volume ( mL) Volume ----> Mass |
Mass/ Density= VOLUME(mL) Volume(mL) x Density= MASS(grams) |
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Chemical Formulas are written to tell us: |
* The number of atoms of each element * Type of compound * The structure of the compound |
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Elemental Composition |
Is the percent composition of a compound which is the mass percent of each element in a compound |
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Percent Composition formula |
PERCENT COMP.= Part(mass)/ Whole(Whole) x 100% |
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Empirical Formula is: |
The simplest formula gives the smallest whole- number ratio of the atoms present in a compound and gives the relative number of atoms of each element present in the compound |
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FORMULA FOR FINDING THE EMPIRICAL FORMULA |
ELEMENTS | GRAMS---->MOL. | DIVIDE By Small | | -est MOL. ___________ |__________________|___________________ | | | | | | | | |
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Molecular Formula is : |
Is the true formula of a compound and it represents the total number of atoms of each element present in one molecule of a compound |
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FORMULA FOR THE MOLECULAR FORMULA |
MF= (EF) n * n= Given Molar Mass/ Molar Mass of EF |
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CHAPTER 8 |
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Coefficients represent what? |
The number of moles and are used to relate the chemicals in an equation when doing stoichometry |
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Stoichiometry |
The area of Chemistry that deals with the quantitive relationships between reactants and products |
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Mole Ratios |
A ratio between the moles of any two substances involved in a chemical reaction NOTE: the coefficients used in mole ratio expressions are derived from the coefficients used in balancing the equation |
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What are mole ratios used for??? |
* To convert the number of moles of one substance to the corresponding number of moles to another substance in a stoichiometry
* Used in the solution of every type of stoichiometry problem |
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Mole Ratio Formula |
MOLE RATIO = Moles Wanted/ Moles Given * Use Coefficients |
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Stoichometry Formula Chart |
| GIVEN| WANTED | |_____________|________|______________| |GRAMS | | | /MM |_____________|________|______________| *G--->MOL. |MOLAR | | | xMM |MASS | | |*MOL.--->G |_____________ |_______ |_____________ | |MOLES | | | _______________|________|_____________| MOL. x MOL. ^ |
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Percent Yield Formula |
% Yield= Actual Yield(Given)/Theoretical yield(Your calculations) x 100 |
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Limiting Reaction |
Is one of the reactants in a reaction and is called the limiting reactant because the amount of it present is insufficient to react with the amounts of other reactants present * Limiting reactant is the amount of product that can be formed |
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Theoretical Yield |
Of a reaction is the calculated amount of product that can be obtained from a given amount of reactant |
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Percent Yield Formula |
PERCENT YIELD = Actual yield/ Theoretical yield * 100 |
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CHAPTER 11 |
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About our Atmosphere... |
* It is a thin layer surrounding us and is critical to life on earth * Is 78% N2, and 21% O2 at sea level, PLUS CO2 and water vapor and noble gas |
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Pollutants |
SO and NO cause rain acid x x * CFC's destroy O3 uv protective layer |
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Average Composition of DRY air |
* 78% N2 * 20.95% O2 |
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Behavior and Properties of Gases |
* Can be compressed greatly * Han expand to fill container uniformly * Has low density compared to liquids and solids * May be mixed-> always homogenous mixtures because always in motion * A confined gas exerts constant pressure on walls of its container uniformly in all directions |
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Kinetic-Molecular Theory (KMT) |
* KMT is based on the motions of gas particles |
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Ideal Gas |
A gas that behaves exactly as outlined by KMT |
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Principle Assumptions of the KMT |
1.) Gas consists of tiny subatomic particles 2.) The distance between particles is large compared with the size of the particles themselves 3.) Gas particles have no attraction for one another 4.) Gas particles move in straight lines in all directions, colliding frequently with one another and with the container wall 5.) No Energy is lost by the collision of gas particles 6.) The average Kinetic Energy for particles is the same for all gases at the same Temp. and its value is disproportional to the Kelvin temp. |
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Gas Properties 4 Quantities define state of a gas are .. |
1.) Quantity in moles or molar mass 2.) Temp. in Kelvin 3.) Volume in Liters 4.) Pressure in atmospheres (usually) |
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Formula for Kinetic Energy |
2 KE= 1/2* Mass * Velocity |
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Pressure |
Force/Unit area |
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Force |
Mass x Acceleration * Force causes something to move a distance D in work F= m xg, units = Newtons force or pounds * Gravity is a weak force |
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Gas Pressure |
The pressure exerted by a gas depends on : - The number of gas molecules present - The Temp. of the gas - The volume in which the gas is confined *The pressure of a gas in a fixed volume increases with increasing temp. |
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Mercury Barometer |
The atmosphere above us exerts a pressure called atmospheric pressure which is measured by a mercury barometer. * A tube of mercury is inverted and placed in a dish off mercury |
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Pressure Units Equivalent to 1 Atmosphere |
1 ATM = 760 Torr = 760 mm Hg = 14.7 IB/in2(psi) = 33.9 ft Water |
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GAS LAWS FORMULA LIST |
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Combined Gas Laws |
P1V1 / T1 = P2V2 / T2
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Boyle's Law |
* T is constant(Pressure goes up and Volume goes down) P1V1 = P2V2 |
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Charle's Law |
* P is constant ( Temp. goes up and Volume goes down) V1 / T1 = V2 / T2 |
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Gay-Lussac's Law |
* V is constant (Temp. goes up and Pressure goes up) P1 / T1 = P2 / T2 |
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STP |
* T = 0 Degrees Celsius = 273.15 K * P = 1 ATM = 760 Torr = 14.7 psi |
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Dalton's Law of Partial Pressure |
P Total = P + P + P ....... a b c |
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Collecting a Gas Sample Over Water |
P Total = P + P + P ATM Gas H2O |
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Avogadro's Law |
* Pressure and Temp. are constant * n = # of Moles V1 / n1 = V2 / n2 |
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Ideal's Gas Law |
*** R = Ideal Gas Constant = 0.082057 L - ATM / Mol. - K PV = nRT |
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Super Combined Gas Law |
P1V1 / n1T1 = P2V2 / n2T2 |
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STP: Mole Mass Volume Relationship |
* 1 MOl. of any gas at STP = 22.414 L = Molar Volume |
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Density of Gases |
* V depends on T and P D = M(grams) / V(liters) * True at STP: D = m(Molar Mass) / V(22.414 L) |
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Variations of the Ideal Gas Law |
* Relationship to Molar Mass: Mols.=mass/ molar mass n = m / M or PV = mRT / M * Rearrange to calculate Molar Mass or even density: M = mRT /PV = DRT /V or m /V = PM /RT = Density |
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Diffusion |
The ability of two or more gases to mix spontaneously until they form a uniform mixture |
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Graham's Law of Effusion |
* a process by which gas molecules pass through a very small orifice from a container at higher pressure one at lower pressure
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