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Calculate the number of grams of sulfuric acid in 0.500 L of battery acid if the solution has a density of 1.28g/mL and is 38.1% sulfuric acid by mass.
Calculate the solubility of zinc hydroxide, Zn(OH)2, in 1.00 M NaOH. Ksp = 3.0 × 10-16 for Zn(OH)2, Kf = 3.0 × 1015 for Zn(OH)42-
assume that a gold atom is shaped like a sphere. an atom of gold has a radius of 156 pm and a mass of 197 amu.
Calculate the equilibrium concentrations of CO2, H2, and H2O at 800 K if only CO and H2O are present intially at concentrations of .119M?
A nugget of pure gold of 4.80 grams is absorbed 284 Joules of heat. if the initial temperature was twenty eight degree Celsius then what was the final temperature of the Au? The specific heat of gold = 0.129 J/(g·°C)?
In an electrolysis cell similar to the one employed in this experiment, a student observed that his unknown metal anode lost 0.238 g while a total volume of 84.90 mL of H2 was being produced.
A source water mineral analysis shows the following ion concentrations in the water: Ca2+ = 70 mg/L, Mg2 + = 40 mg/L, and HCO3- = 250 mg/L as CaCO3. Determine the water's carbonate hardness, noncarbonated hardness, and total hardness.
what is the mass percent ch3oh of a 0.256 m ch3ohaq
Draw (2R,3R)-2-bromo-3-phenylpentane in the conformation from which it is most likely to undergo E2 elimination to give 3-phenyl-2-pentene.
the reaction must progress forward to attain equilibrium. The richer a reaction mixture is in product the higher its Q value is. The value of K does not change as a reaction progresses toward equilibrium.
ammonia gas is produced by reacting hydrogen gas with nitrogen gas. to produce 856 g of ammonia gas using air as your
Categorize each phrase below as being relevant to ionic bonding, covalent bonding or metallic bonding. 1. electron transfer 2. Nonmetal with nonmetal 3. Alloy 4. separate molecules 5. metal with metal 6
What is the maximum amount of ethanol (in millimoles) that could theoretically be produced under the following conditions?
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