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47 Cards in this Set
- Front
- Back
homogeneous
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all mixed together equally, all in one phase
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Heterogeneous
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orange juice with pulp, liquid + solid
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Density=
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mass/volume
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Celsius to Fahrenheit
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F = (9/5)C + 32
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precision
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how close measurements in a series are to eachother
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accuracy
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how close a measurement is to the actual value
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kinetic energy
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energy due to motion
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potential energy
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energy due to position
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K to C
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C = K - 273.15
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Law of Conservation of Mass
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Mass is conserved in chemical reactions
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Law of Constant Composition
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compounds compositions are the same ANYTIME, ANYWHERE
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Law of Multiple Proportions
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Elements combine in specific rations every time
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1 mole (mol)
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6.022 x 1023
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molar mass
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the mass in grams of one mol of substance
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mass % =
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mass of atoms of element/mass of all atoms x 100
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find empiricle formula of compound with C=44.77% H=7.52% and O=47.71%
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C5H10O4
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s
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solid
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l
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liquid
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g
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gas
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aq
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aqueous
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limiting reactant
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reactant that runs out first and determines final amount
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theoretical yield
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max. possible yield of products, predicted by the balanced equation and reactant quantities
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Theoretical yield of ammonia in the reaction of 25.0 g N2 and 6.00 g H2?
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Theoretical Yield = 30.4 g NH3
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Percent yield =
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actual yield/theoretical yield
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41.5 g bromobenzene from 25.2 g benzene and excess bromine, percent yield?
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81.90%
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base
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yield OH- in water
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Isotope
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atoms with same number of protons, but different numbers of NEUTRONS
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Empirical Formula
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Shows the simplest integer ratio of atoms of each element in a compound
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Molecular Formula
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Shows the number of Atoms of ach element in a molecule
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Structural Formula
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Shows the connectivity of the atoms in a molecule
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Formulas of hydrogen peroxide
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Empirical Formula: HO Molecular Formula H2O2
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Acid
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Yield H+ ions in water
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Binary Aqueous Acids
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acid = 2 elements (aq) = in water
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Hydrocarbons
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contain only carbon and hydrogen
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Alkanes
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hydrocarbons with only single bonds
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Compound
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matter composed of two or more different elements chemically bonded together
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mixture
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two or more substances that are physically intermingled
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What mass of iron(III) oxide will be produced if 12.3 g of iron react with an excess of oxygen according to the reaction, 4F(s) + 3O2(g) --> 2Fe2O3(s)
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a) 4.4 g b) 8.8 g c) 16.7g d) 17.6 g e) 35.2 g
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isomers
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compounds with the same molecular formula, but with different properties (shape, etc.)
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titrant
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a solution of accurately known concentration
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analyte
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a solution of unknown concentration
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equivalence point
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exact titrant volume required to completely react with the analyte
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end point
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the titrat volume slightly in excess of that required to completely react with the analyte
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metal activity series
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Li, K, Ba, Ca, Na, Mg, Al, Mn, Zn, Cr, Fe, Cd, Co, Ni, Sn, Pb
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reversible reaction
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reaction that proceeds simultaneously in both directions
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equilibrium
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the forward reaction and the reverse reaction proceed at equal rates
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combustion reactions
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2C4H10 + 13O2 ----> 8CO2 + 10H2O
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