Part C You carefully weigh out 15.00 g of CaCO3 powder and add it to 60.75 g of HCI solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 69.60 g. The relevant equation is CACO3 (s) +2HCI(aq)→H2O(1) + CO2(g) + CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA Value Units Submit

Part C You carefully weigh out 15.00 g of CaCO3 powder and add it to 60.75 g of HCI solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 69.60 g. The relevant equation is CACO3 (s) +2HCI(aq)→H2O(1) + CO2(g) + CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA Value Units Submit

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 38CR

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
As part of the aspirin synthesis lab the orgo students also had to perform the following calculation to demonstrate their knowledge. Are you able to help them work this out? Saponification is a process in which soap is produced from the chemical reaction between animal fat (triglycerides) and a strong base such as KOH. An example of such balanced chemical reaction is shown here: C51H98O6 + 3KOH → C3H5(OH)3 + 3C16H31O2K (Triglyceride) (Soap) if during the saponification reaction 231.5 g of C51H98O6 is mixed with 231.5 g of KOH and 160 g of soap is produced. Calculate the theoretical yield of soap C16H31O2K and indicate who is the limiting reactant. (Provide your answer to 2 decimal places) Calculate the percent yield for this reaction (Provide your answer to 1 decimal place) *Show ALL steps and mathematical equations involved in your calculations to help the orgo students. Remember to label all…
Solutions of cyanide salts are still widely used in the extraction of gold metal from its ores. It is thereforenecessary to regularly monitor the quality of the reagents used to make such solutions.The purity of a sample of solid potassium cyanide is determined as follows: 5.00 g of the impure potassium cyanide is weighed off, and quantitatively transferred into a100.00 mL volumetric flask, dissolved and made up to the mark. A 10.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.200 MKMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns abright pink due to the presence of excess permanganate ions. The average titration value is 20.69 mL of the KMnO4 solution.The reaction stoichiometry is as follows: 2KMno4(aq) + 3KCN(aq) + H2O(l) → 2MnO2(s) +3KOCN(aq) + 2KOH(aq) ૝1.1 Determine the percentage purity of the potassium cyanide.
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 results
Combustion of hydrocarbons such as undecane (C11H24) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid undecane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.310kg of undecane are burned in air at a pressure of exactly 1atm and a temperature of 18.0°C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. = L
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5.127 Photosynthesis produces glucose (C6H12O6) and oxygen from carbon dioxide and water:
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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)
Sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.8×10−3M in Ca2+ and 1.1×10−3M in Mg2+ and that the average capacity of a washing machine is 24.5 gallons of water. 1gallon=3.785L If the detergent requires using 0.61 kg detergent per load of laundry, determine what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water. Express your answer in percent to two significant figures.
Sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.8×10−3M in Ca2+ and 1.1×10−3M in Mg2+ and that the average capacity of a washing machine is 24.5 gallons of water. 1gallon=3.785L If the detergent requires using 0.61 kg detergent per load of laundry, determine what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water.
The sugar content of a wine is determined five times, and the following results obtained: 150, 155, 155, 152 en 144 g/L. Determine with 90% confidence if the 5th value (144 g/L) must be excluded (outlier) or included (not outlier) in further calculations

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