Sem. 1 Final Exam

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Relatively slow rates of chemical reation are associated with which of the following?
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Strong bonds in reactant molecules
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Standard enthalpy change for Na2O + H2O= 2NaOH
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-150 kJ
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Planar configuration
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BCl3
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N2 + 3H3= 2NH3
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change in G, H, and S are negative
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change in H for I2 + 3Cl2= 2ICl3
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-390 kJ
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two unshared pairs of electrons on central atom
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H2S
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Molecule with only one double bond
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C2H4
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Molecule with the largest dipole moment
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H2O
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trigonal pyramidal geometry
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PH3
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change in H for 3C2H2= C6H6
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-607 kJ
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most ionic compound
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CaCl2
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NH4SCN
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change in G negative, change in H and S positive
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most positive oxidation number
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SO2
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compound that shows resonance
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SO2
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PF5 does not have
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d2sp3 hybridization
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decrease in entropy
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formation of a crystalline solid from a supersaturated solution
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electrons shared by hydrogen and oxygen
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spend more time around oxygen
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decreasing bond polarity
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HF HCl HBr HI HAt
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most ionic elements
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CsF
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number of structures for NO3-
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3
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molecule that violates octet rule
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SF4
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number of electrons on FCl3
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6
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bond energy for CH4 + 4F2= CF4 + 4HF
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-1924 kJ
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shape of AX5 with one nonbonding pair of electrons
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square pyramidal
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shape of AX3 with two lone pairs of electrons
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T-shaped
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shapes of NH3 and BF3
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trigonal pyramidal and trigonal planar
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molecule that is nonpolar
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CF4
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polar molecule
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PCl4F
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square planar hybridization
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sp3d2
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PCl5 hybridization
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sp3d
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negative change in S
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compressing one mole of Ne at constant temperature from .5 to 1.5 atm
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first law of thermodynamics
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energy cannot be created or destroyed but must be conserved
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second law of thermodynamics
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entropy of the universe is increasing
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specific heat capacity
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amount of energy required to raise one gram of a substance one degree Celsius
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heat released when 9.25 moles of Fe is reacted with oxygen
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-3820 kJ
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change in H for P4O10 + 6PCl5 =10Cl3PO
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-610 kJ
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formula for P2O5
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diphosphorus pentoxide
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kinetic molecular theory does not say
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gas particles move at speeds close to the speed of light
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Cu65 isotope in nature
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25%
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Average atomic or molecular speed closest to N2 molecules at 0 C and 1 Atm
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CO
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greatest density at 0 C and 1 Atm
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Xe
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Values that decrease when ideal gas is cooled by 25 degrees
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average distance between molecules and average speed of molecules
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percent of CaCO3 by mass in limestone
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35%
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safest and most effective way to treat an acid splash on skin
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flush affected area with water and then with a dilute NaHCO3
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moles of HI needed to produce 2.5 moles of I2
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5
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why does water boil at a lower temperature on a mountain
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equilibrium water vapor pressure equal the atmospheric pressure at a lower temperature
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partial pressures of gasses
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He less than Ne less than Ar
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gas that deviates most form ideal behavior
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SO2
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the a coefficient in van der Waals equation
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forces of attraction between molecules
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how many protons, neutrons, and electrons are in Sr-90
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38, 52, 38
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Quantum numbers of ground-state gallium
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4,1,1,1/2
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pauli exclusion principle
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indicates that an atomic orbital can hold no more than two electrons
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dissolves in water to form a colorless solution
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ZnCl2
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not true about halogens
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iodine liberates free bromine from a solution of bromide ion
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barium sulfate is least soluble in a .01 molar solution of what
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Al2(SO4)3
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what color is the flame when a solution of sodium chloride is vaporized in a flame
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yellow
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use of a visible-light spectrophotometer
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determining the concentration of a solution of Cu(NO3)2
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based on ionization energies in chart, element X is what
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Al
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what happens to atomic radius as atomic number increases from 11-17
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decreases
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Rutherford’s gold atom experiment
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neutrons are at the center of an atom
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yellow precipitate forms when NaI is added to what
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Pb
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not soluble in water but soluble in dilute hydrochloric acid
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Mg(OH)2
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what will separate Pb from other ions
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dilute HCl solution
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contains exactly two unpaired electrons
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S
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contains only one electron in the highest occupied energy sublevel
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Ga
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purple in aqueous solution
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KMnO4
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white and soluble in water
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KCl
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isoelectronic elements
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Mg, Ca, Sr
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greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90 degrees C to 30 C
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KNO3
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which property decreases across the periodic table form sodium to chlorine
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atomic radius
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why is there a different nuclear charge on Na and Ne
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Na has a higher neutron-to-proton ratio than Ne
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sodium chloride is least soluble in what
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CCl4
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all halogens are
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diatomic
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least soluble in water
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BaCO3
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with chart, which ions could be present in solution at a concentration of .1 M
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Na
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what pure white crystalline solid dissolves in water to yeild a base and liberate gas when acid is added to it
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K2CO3
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mixture is made by adding AgNO3 to Na2CrO4, what does it look like
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yellow before, red precipitate
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precipitate made when AgNO3 is added to Na2CrO4
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Ag2CrO4
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compare Cl zero and Cl negative
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Cl zero atom contains fewer electrons than the Cl negative ion
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increasing atomic radius
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Na, K, Rb
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quantum numbers for 3d^4
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3,2,-1,1/2
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greatest difference between its first and second ionization energies
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potassium
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frequency of blue light
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7.5 times 10 to the 14
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wavelength of sodium light
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5.9 times 10 to the -7
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energy of photon of red light
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2.84 times 10 to the -19
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ionic equation for NaCl +AgNO3= NaNO3+ AgCl
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Ag + Cl= AgCl
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insoluble in water
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CaCO3
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soluble in water
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K2S
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precipitate formed from ammonium phosphate and calcium sulfate
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Ca3(PO4)2
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orbital designation for an electron with n=4 and L=3
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4f
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electron configuration that isn’t possible
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1s^2 2s^2 2p^6 3s^3 3p^4
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not possible configuration for an atom in excited state
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1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2
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increasing atomic size
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Br, As, V, Sc, K
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electron affinity equation
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atom + electron= ion
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metallic elements
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low ionization energies
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formula for Hg2Cl2
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mercury 1 chloride
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not a correct formula
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KCr2O7
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sulfate polyatomic ion
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SO4 negative 2
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empirical formula of CH2 and mass of 83.5 what is molecular formula
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C6H12
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empirical formula for compound made of carbon and hydrogen that is 14.3% H
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CH2
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gram molar mass of Al(NO3)3
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213
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2 L container will hold 4g of what
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CO2
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8g of N2H4 and 92g of N2O2 mixed, how much H2O is made
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9 grams
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propane burns in excess oxygen, what is coefficient of O2
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7
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volume of H2 when excess Mg is added to .4 M HCl
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448 mL
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volume of O2 required to react with excess CS2 to make 4 L of CO2
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12 L
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mass of CuSO4 with water required to make .1 M copper sulfate
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6.2 grams
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compound with 1.1 mole of K, .55 moles of Te and 1.65 moles of O
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K2TeO3
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partial pressure of SO2 in flask
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160 mmHg
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greatest rate of effusion through pinhole
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Ne
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mass ratio of chromium to oxygen closest to 1.6 to 1
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CrO2
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pressure of gas at 27 C
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.6 Atm
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change the boiling point of a liquid
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smaller container, more moles, higher altitude
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info needed to calculate molarity
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molar mass of sucrose
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formula for hydrocarbon with 1.88 density
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CH2
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with info, density of sample is
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2 grams per cm
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what gas effuses at half rate of NH3
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Cl2
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mass of Au made when .05 moles of Au2S3 is reduced with excess H2
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19.7 grams
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coefficient of O2 for C10H12O4S +O2= CO2 + H2O
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12
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what happens to gas in tank when more oxygen is added
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volume of gas increases
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empirical formula for 62.2% Hf and 37.4% Cl
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HfCl3
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pressure of flask of NH4NO3 at 400 K
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1 Atm
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percent water in hydrate Na2Co3 times 10H2O
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63%
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height of column of water of barometer
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33.9
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object moves from moon to Earth
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mass will stay same and weight will increase
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formula for Hydrogen arsenide
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H3As
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when real gas is most like ideal gas
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low pressure and high temperature
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ideal gases
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have no volume or attractive forces between them

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