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A 1.00 g sample of enriched water, a mixture of H2O and D2O, reacted completely with Cl2 to give a mixture of HCl and DCl. The HCl and DCl were then dissolved in pure H2O to make a 1.00 L solution. A 25.00 mL sample of the 1.00 L solution was reacted with excess AgNO3 and 0.3800 g of an AgCl precipitate formed. What was the mass % of D2O in the original sample of enriched water? Atomic masses (g/mol): H = 1.0, D = 2.0, O = 16.0, Cl = 35.5, Ag = 107.9
Consider the reaction CaCN2 + 3 H2O → CaCO3 + 2 NH3 . How much CaCO3 is produced if 47.5 moles NH3 are produced
What is the rate law for step 1 of this reaction? ((Express your answer in standard Mastering Chemistry notation.
Provide the structure of an aromatic compound with seven carbon atoms. Draw the molecule on the canvas by choosing buttons from the Tools (for bonds)
Determine which species is present in the lowest concentration in 0.10 M H3A solution?
A mixture of CaCO3 and CaO weighing 0.680 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.489 g.
find the molarity when 7.85 moles aluminum chloride are dissolved in enough water to make a total of 600. mL
A 100.0-mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. What is the pH of the solution after 100.00 mL of acid have been added to the ammonia solution?Kb = 1.8 × 10-5.
Help me understand specifically why the dissociated phosphate ion would prefer to bond with cations like Al and Zn. I think I know why but help me better understand.
4NH3 + 5O2 yields 4NO + 6H2O Given 1.50g of NH3 reacts with 2.75g of O2 which is the limiting reactant?
if you burn 51.8 g of hydrogen and produce 463g of water, how much oxygen reacted?
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.676 grams of iron and 13.1 mL of 0.448M copper(II) sulfate react to form as much product as possible,
the reaction rate does not change when [B] increases from 1 M to 2 M. Which of the following is the correct rate law for the reaction?
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