Given the following balanced reaction 4KNO3 (aq) → 2K2O (s) + 2N2 (g) + 502 (9), fill in the blanks for the road maps for the following situations: a) Moles of O2 produced from the decomposition of moles of KNO3. Conversion Factor: b) Mass of N2 produced when moles of K20 is produced. Conversion Factor 1: Conversion Factor 2: c) Mass of KNO3 decomposed when grams of K20 is produced. Conversion Factor 1: Conversion Factor 2: Conversion Factor 3:

Given the following balanced reaction 4KNO3 (aq) → 2K2O (s) + 2N2 (g) + 502 (9), fill in the blanks for the road maps for the following situations: a) Moles of O2 produced from the decomposition of moles of KNO3. Conversion Factor: b) Mass of N2 produced when moles of K20 is produced. Conversion Factor 1: Conversion Factor 2: c) Mass of KNO3 decomposed when grams of K20 is produced. Conversion Factor 1: Conversion Factor 2: Conversion Factor 3:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 156QRT: Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose....

See similar textbooks

Similar questions

When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
Given the following balanced reaction 4KNO3 (aq) → 2K2O (s) + 2N2 (g) + 5O2 (g), fill in the blanks for the road maps for the following situations: A) moles of O2 produced from the decomposition of moles of KNO3. blank-blank-converrsion factor-blank b) Mass of N2 produced when moles of K2O is produced. blank-blank-blank-conversion factor 1 blank - conversion 2 - blank c) Mass of KNO3 decomposed when grams of K2O is produced. blank-blank-blank-blank- conversion factor1-blank - conversion factor2-blank - conversion factor3-blank have to this where it say blank one each blank that one belong it. mole of kno3 , mass kno3- mass ration - molar mass- mole o2-moles n2-mass n2- mass k20- moles k2o
Given the following balanced reaction, Fe2O3+3C-->2Fe+3CO if 1140 of fe2o3 were reacted with ecess c, what would be the percent yield for the reaction if 455g of CO were actually collected? density fe2o3=5.24g/cm3, density of co is 1.14kg/m3
An industrial-scale process for making acetylene consists of the following sequence of operations: CaCO3 → CaO + CO2limestone lime carbon dioxideCaO + 3 C → CaC2 + CO calcium carbide carbon monoxideCaC2 + 2 H2O → Ca(OH)2 + C2H2 calcium acetylene hydroxide What is the percentage yield of the overall process if 2.32 metric tons C2H2 is produced from 10.0 metric tons limestone (1 metric ton 5 1000 kg)?
Potassium chromate, a bright yellow solid, is produced by the reaction of solid chromium ore (FeCr2O4) with solid potassium carbonate and gaseous oxygen at high temperatures. The other products of the reaction are solid iron (III) oxide and gaseous carbon dioxide. If you use 169.0g of chromium ore, 298.0g of potassium carbonate and 75.00g of oxygen in a sealed reaction vessel, what is the limiting reagent? Give the theoretical yield of potassium chromate, in grams, for each one.
The following is the balanced equation for the combustion of butanol in oxygen:C4H9OH(g) + 6O2 --> 4 NO(g) + 6H2O(g) a. How many grams of butanol must be burned to produce 18.50g of carbon dioxide? b. How many grams of water are also produced? c. How many grams of oxygen are needed to produce 18.50g of carbon dioxide? d. Use the results from a, b and c to show this reaction obeys the law of conservation of mass.
In a blast furnace, iron (III) oxide is used to produce iron by the following (unbalanced) reaction: Fe2O3 (s) + CO(g) -> Fe(s) + CO2(g) If 4000 g of Fe2O3 is available to react, how many moles of CO are needed?
Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 60.2% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 65000kg coal that is 0.30 mass % sulfur?
Given the following Reaction: 2C5H10O2 + 13O2 → 10CO2 + 10H2O. If 3.95 moles of O2 are reacted with an EXCESS of C5H10O21. a. a. How many moles of C5H10O2 are used? b. How many moles of H2O are produced? c. How many moles of C5H10O2 would you need to use to produce 4.42 moles of CO2 given that there is an excess of O2?
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)?
Write the balanced chemical equation for the combustion of the fuel in O2(g), with CO2(g) and H2O(g) as products. Adjust the coefficients of the balanced equation so that there is one mole of the fuel. The coefficient on O2 may be fractional, e.g., 13/2.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS