Use the equation 6KI (aq) + 8HNO3 (aq) → 6KNO3 (aq) + 2NO (g) + 312 (s) +4H20 (). If 17.77 mL of 0.860 M KI are reacted, how many molecules of I2 will be produced? Answer using Canvas's scientific notation, "e". For example, 5.2x103 would be entered "!
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- A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.An unspecified amount of sulfuric acid is added to 1.19 g of solid barium chloride, then water is added to form a solution with a total volume of 1.72 L. Assuming the reaction goes to completion and that the volume does not change during the reaction, what is the molarity of the solution with respect to barium sulfate? You may assume that barium chloride is the limiting reactant. (3 sf) The pertinent balanced chemical equation is: BaCl2 (aq) + H2SO4 (aq) à BaSO4 (s) + 2 HCl (aq)Hydrobromic acid dissolves solid iron according to the following reaction: Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g) What mass of HBr (in g) would you need to dissolve a 2.8-g pure iron bar on a padlock? Express your answer using two significant figures. What mass of H2 would be produced by the complete reaction of the iron bar? Express your answer using two significant figures.
- One of the reactions in the Solvay Process involves the reaction of calcium oxide with water toproduce slaked lime (calcium hydroxide).CaO(s) + H O2 (l) - Ca(OH)2 (s)A lab technician performs the experiment and uses 54.8 g of calcium oxide to react with a setamount of water. When the reaction is completed, the technician uses a filtration apparatus tocollect the mass of calcium hydroxide produced. The following data is recorded:Mass of filter paper: 1.24 gMass of filter paper and solid: 68.04 g What is the theoretical mass of calcium hydroxide that is predicted to be produced? What mass of precipitate was collected in this experiment? What is the percent error? Comment on the validity of the resultsA student performs the titration of hydrochloric acid with sodium hydroxide. A 20.00 mL aliquot of the HCl solution required 30.50 mL of a 0.150 mol L-1 NaOH solution to reach the end point in the titration using a phenolphthalein indicator. Write the balanced molecular equation for this reaction AND determine the concentration of the original hydrochloric acid solution. Give your answer to the correct number of significant figures.Hydrobromic acid dissolves solid iron according to the following reaction: Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g) A.) What mass of HBr (in g) would you need to dissolve a 2.6−g pure iron bar on a padlock? Express your answer using two significant figures. B.)What mass of H2 would be produced by the complete reaction of the iron bar? Express your answer using two significant figures.
- A chemical reaction occurs in a closed system to observe and test the Law of Conservation of Mass.A piece of copper metal is placed in a silver nitrate solution in an Erlenmeyer flask. The flask is stoppered, weighed, and observed.The reaction that occurs is Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s).Once the chemical reaction was complete, the system was weighed again.The mass of the reactants is measured to be a total mass of 122.8 g.After the reaction is complete, what will be the mass of products formed?Record only your final answer with the correct number of significant digits and proper units.. An aqueous solution of sodium carbonate, Na2CO3, is titrated with strong acid to a point at which two H1 ions have reacted with each carbonate ion. (a) If 20.0 mL of the carbonate solution reacts with just 40.0 mL of 0.50 Macid, what is the molarity of the carbonate solution? (b) If the solution contains 5.0 percent by mass sodium carbonate, what is the density of the solution? (c) Suppose that you wanted to prepare a liter of an identical solution by starting with crystalline sodium carbonate decahydrate,Na2CO3?10H2O, rather than with solid Na2CO3 itself. How much of this substance would you need?Hydrochloric acid can dissolve solid iron according to the following reaction.Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g) a) What minimum mass of HClHCl in grams would you need to dissolve a 2.4 gg iron bar on a padlock? Express your answer using two significant figures. B) How much H2H2 would be produced by the complete reaction of the iron bar? Express your answer using two significant figures.
- The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. Suppose 48.0mL of dioxygen gas are produced by this reaction, at a temperature of 100.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.(5) A 25.0-mL sample of 1.00 M Calcium nitrate solution, Ca(NO3)2, is reacted with 125.0 mL of 0.300 Mpotassium iodate, KIO3, and calcium iodate precipitate, Ca(IO3)2(s), is produced according to the following equation. Ca(NO3)2(aq)+ 2KIO3(aq)-->Ca(IO3)2(s)+ 2KNO3(aq) (a)Determine the limiting reactant. (b)How many grams of Ca(IO3)2is produced if the yield is 100%? (c)What is the percent yield ifthe actual yield of Ca(IO3)2is6.72 g ?