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A solution of Ba(OH)2 and a solution of H2SO4 are mixed. Water and precipitate of BaSO4 are formed.
Lead(II) sulfide reacts with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?
a 5.00 mL sample of isopropyl alcohol has a mass of 3.930 g when measured at 20 degrees Celsius? what is the specific gravity of isopropyle alcohol?
A chemist burns 160g of aluminum oxygen to produce aluminum oxide. She produces 260g of aluminum oxide. Write a balanced equation and calculate the theoretical and percent yield
he maximum contaminant level (MCL) for barium (Ba) in drinking water is 2.0 mg/L. Barium can combine with sulfate (SO42-) to form BaSO4(s), which precipitates out of the water. This can be achieved by adding Na2SO4
The normal boiling point of the liquid is 425 K. Liquid, X, and Y are all in equilibrium at 342 K and 1800 bar. Tc = 571K, Pc= 46 bar
what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.184 J/g×K and the molar mass of ethanol is 46.07 g/mol.
When 1.28 mg of hydrogen peroxide decomposes in the presence of manganese dioxide to form water and oxygen, how many miligrams of each are produced?
a 1.00 g sample of an alloy of copper and aluminum was reacted with hydrochloric acid , and 85.0 mL of hydrogen gas (measured atSTP) was produced.
what is the molar concentraion of the salt solution formed n this reaction? B. what is the molar concentraion of the excess reactant once this reaction has finished?
The human body obtains 1091 kJ from a candy bar. If this energy were used to vaporize water at 100°C, how much water in liters could be vaporized? (Assume that the density of water is 1.0 g/mL.)
Account for the fact that H3C-Cl (dipole moment 1.94D) and H3C-F (dipole moment 1.82D) have almost identical dipole moments, even though fluorine is considerably more electronegative than chlorine.
If you have .200 mL of methyl salicyate (density=1.184 g/mL)(molar mass=152.15 g/mol) how many moles do you have?
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