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An 11.79 sample of mo2o3(s) is converted completely to another molybdenum oxide by adding oxygen. the new oxide has a mass of 12.578g. What is the Empirical formula of the new oxide
electrons are ejected with a kinetic energy of 3.54x10^-19 J. What is the work function of the metal in joules?
mass is obtained in the reaction, what mass of S2O3^2- was present initially, assuming the reaction went to completion? the density of the HSO3^- solution is 1.45 g/cm^3
a.) Available Electrons (AE) b.) Needed Electrons (NE) c.) Geometry Description d.) Number of sigma bonds e.) bonding description f.) lewis dot structure
Cerium is often used as a reducing agent. Although it is expensive, it has a high stabile and constant value of E^ o over a PH range from 0 to 7.
Suppose that coal of density 1.5 g/cm3 is pure carbon. (It is, in fact, much more complicated, but this is a reasonable first approximation.)
A specific brand of gourmet chocolate candy contains 7.00 g of dietary fat in each 22.7 g piece. How many kilograms of dietary fat are in a box containing 4.00 lb of candy?
"Given the following standard reduction potentials, E°redAl3+/Al = -1.66 V. E°redCr3+/Cr = -0.74 V.
A patient is given 5.5 x10^-2 mg of technetium-99 m, a radioactive isotope with a half-life of about 6.0 hours.How long untilth radioactive isotope decays to 6.0 x10-3 mg? (assume no excretin of the nucelotibe from the body.) Answer is in T =hours.
What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that is buffered at a pH of 4.55 and has a freezing point of -2.0 °C.
If the chemist mistakenly makes 275 mL of solution instead of the 200 mL, what molar concentration of sodium nitrate will the chemist have actually prepared?
34.62 mL sample of .1510 molar NaOH was needed to completely neutralize 50 mL of an H2SO4 solution. what is the concentration of the origional sulfuric acid solution?
Assuming that the total pressure of the gases is 1.52 and that their mole ratio is 94 : 4.0 : 1.5 : 0.50, calculate the partial pressure (in atmospheres) of each gas.
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