A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H20. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. To obtain the exact answer, use the molar of C being equal to 12.01 g; the molar mass of H 1.010 g; the molar mass of O 16.00 g. In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. Hint 1: Look up the example problem in the next, last question. Hint 2: Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. The mass of carbon is g. The mass of hydrogen is g. The mass of oxygen is g.

A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H20. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. To obtain the exact answer, use the molar of C being equal to 12.01 g; the molar mass of H 1.010 g; the molar mass of O 16.00 g. In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. Hint 1: Look up the example problem in the next, last question. Hint 2: Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. The mass of carbon is g. The mass of hydrogen is g. The mass of oxygen is g.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter22: Organic And Biological Molecules

Section: Chapter Questions

Problem 157CP

See similar textbooks

Similar questions

Please help with this question: Thanks!!! C15H24 (39.288g) was oxidized to C9H6O6, using an excess of oxidizing agent. Calculate the theoretical yield of the organic product a) in moles, and b) in grams.
Give the theoretical yield, in moles, of CO2 from the reaction of 0.60 moles of C8H18 with 40.00 moles of O2. 2C8H18+25O2 ---> 16CO2 + 18H2O
Urea, CH4N2O, is produced by the reaction between ammonia and carbon dioxide, as shown by the followingequation. 2NH3 + CO2 → CH4N2O + H2O a. Calculate the quantities, in kilograms, of NH3 and CO2 that should combine to produce 6.0 kg of urea.NH3 _______________ kgCO2 _______________ kg b. How many kilograms of water will be produced as the side product in this process?H2O _______________ kg
Calcium peroxytoctahydrate is synthesized according to the following reaction. During the synthesis based on 3.5 g calcium carbonate, 7.5 mL of 18% HCl with a density of 1.19 and 5.5 mL of 25% NH3 with a density of 0.91 were used, and further hydrogen peroxide and excess water were added to the medium. Since 2.35 g of calcium peroxytoctahydrate is obtained in this way, what is the% yield of the experiment? (HCl: 36.5 g/mol; NH3: 17 g/mol; CaCO3: 100 g/mol; CaO2.8H2O: 216 g/mol) CaCO3 + 2HCl 2NH3 + H2O2 + 7H2O → CaO2.8H2O + CO2 + 2NH4+ + 2 Cl-
A sample of an industrial waste water is analyzed and found to contain 16.5ppb Fe2+. How many grams of iron could be recovered from 1.81×103 kg of this waste water? Answer:_______ grams Fe
is In the preparation of acetylsalicyclic acid, salicylic acid is the limiting reagent.
18.2 Balance the following chemical equation for the stoichiometric combustion of methane with oxygen. ____ CH4(g) + ______O2(g) ⟶ ______ CO2(g)+ ______H2O(g) What are the coefficients for O2(g) and CO2 (g)?
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) A. What is the %m/m of the solution? B. What is the molarity of the solution? C. What is the mole fraction of the solvent?
0.004 C8H7NO3, 15mL ethanol, 0.002mol NaBH4 was used. HCl was used to acidify. It was then extracted with ether. Then it was dried and a mass of 0.32g was obtained. What is the balanced equation of this synthesis, and what is the limiting reagent?
How many kg of Co2 are produced when 1.00 gallon of octane (C8H18, density = 0.703 g/mL) is completely combusted in the presence of O2 to form CO2 and H2O?
Balance the equation below such that it has the smallest, whole-number coefficients. CH3CH2CH2CH2OH + O2(g) ® CO2(g) + H2O(g)
A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)