Sem. 1 Final Exam – Flashcards
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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 |