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Determine the molarity of a solution prepared by dissolving 0.198 g of "KHP" (C8H5O4K) in enough water to make 125 mL of solution.
When the solution is found and titrated with aqueous sodium hydroxide, the endpoint is reached after the addition of 27.80 mL of base solution. How many moles of NaOH reacted? What is the concentration of the NaOH?
Calculate the number of carbon atoms in 4.56 grams of ethanol (CH3CH2OH).
Calculate the number of ATPs generated from the metabolic oxidation of the four carbons of acetoacetyl-CoA to CO2. Now consider the homolog derived from oxidation of an odd numbered carbon chain
If 159 of wet is collected over water at 24 and a barometric pressure of 737 , how many grams of have been consumed.
calculate the number of excess reagent units remaining when 188 PbS formula units and 279 O2 molecules react?
If 5.78 mol of ethane (C2H6) undergo combustion according to the unbalanced equation C2H6 + O2 = CO2 + H2O how much oxygen is required?
At 25 0C the density of a 50 % (by mass) ethanol/water solution is 0.914 g/cc. Given that the partial molar volume of water in the solution is 17.4 cc/mol.
When 2.0 mol of CO2(g) is placed in a 5.0-L closed container andheated to a particular temperature, the equilibrium concentration of CO2(g) is measured to be 0.039 mol/L. Use an ICE table to determine the equuilibrium concentrations of CO(g) and O..
You have a 48.9 g sample of water at the temperature of -60.0 degrees celcius. How much energy is required to: a) heat the ice to 0 degrees celcius
Find the pH of a solution prepared by dissolving all of the following compounds in one beaker and diluting to a volume of 1.00 L: 0.180 moles acetic acid (pKa=4.75), 0.180 mole sodium acetate
sulfur dioxide is an unwelcome result of burning soft coal in power plants. Some of the sulfur dioxide ends up as sulfuric acid ( H2SO4) in acid rain.
Brominated biphenyls (PBB) is created through an electrophilic aromatic bromization out of the hydrocarbon biphenyl.
A certain substance has a molar heat of vaporization of 31.6 kj/mol. How much of the sunstance is in a sample that requires 57 kj to vaporize.
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