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A .8102-g sample of impure Al(CO3)3 decomposed with HCl; the liberated CO2 was collected on calcium oxide and formed to weigh .0515g. Calculate the percentage of aluminum in the sample.
Calculate the density of N2 at STP, (a) using the ideal-gas law and (b) using the molar volume and molar mass of N2.
1 oz of gold (density=19.3 g/ml) can be hammered into a sheet which would cover a 1.00 x 10^2 ft^2 area what is the thickness.
What changes would I make in my experimetal procedure to determine the rate law for the oxidation of red dye by sodium hypochlorite
The bond in molecular iodine is quite weak, and hot iodine vapor contains a proportion of atoms. When 1.00 g of I2 is heated to 1000 K in a sealed container of volume 1.00 L
Calculate the specific heat per mole in J/mol°C for each noble gas.comment on the values you obtain. why was the question included. can someone show me how to solve this problem step by step.
Calculate the average kinetic energies of the CH4 and N2 molecules at 286 K and 556 K?
silver chloride can dissociate into Ag+ and Cl- species. This inhomogenous equilibrium has K=1.8x10^-10. What is the concentration of Ag+ in solution at equilibrium?
the maximum velocity of the ejected electrons is 3.45 multiplied by 105 m/s. Calculate the binding energy of electrons to the magnesium surface.
If propyl amine was dissolved in ether along with biphenyl, what is the best way to separate the compounds
A certain substance has a heat of vaporization of 37.43 kJ/mol. At what Kelvin temperature will the vapor pressure be 7.00 times higher than
An experiment requires 42.0 g of ethylene glycol, a liquid whose density is 1.114 g/mL. Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder.
what mass of limestone must have dissolved if 3.05x10^10 kg of calcium hydrogen carbonate was produced? CaCO3(S)+H2CO3(aq)->Ca(HCO3)2(aq)
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