Solve a 1. Waste Organic material is to be burned in a waste to energyfacility. The chemical equation for the material is C6H1005a) Calculate the stoichiometric Oxygen necessary for thecombustion of this materialb) Calculate the stoichiometric air requiredc) If the combustion process is carried out at 50% excess air inorder to assure complete combustion, recalculate (a) and (b)above

1. Waste Organic material is to be burned in a waste to energy facility. The chemical equation for the material is C6H1005 a) Calculate the stoichiometric Oxygen necessary for the combustion of this material

1. Waste Organic material is to be burned in a waste to energy facility. The chemical equation for the material is C6H1005 a) Calculate the stoichiometric Oxygen necessary for the combustion of this material

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter26: Biodiesel

Section: Chapter Questions

Problem 3Q

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A fuel composed entirely of methane (CH 4 ) and nitrogen (N 2 ) is burned withexcess air. The flue gases analyze 7.5% CO 2 , 7% O 2 and the remainder, N 2 .Calculate:(a) percentage of excess air(b) analysis of fuel gas(c) analysis of flue gas (wet basis)
A chemical manufacturer produces ethylene oxide by burning ethylene gas with air in the presence of catalyst. If the conditions are carefully controlled, a substantial fraction of ethylene remains unconverted and some is completely oxidized to form carbon dioxide and water. Formation of carbon monoxide is negligible. After the gases leaving the absorber is as follows: 9.6%CO2, 3.0%O2 and 6.4% ethylene. Of the ethylene entering the reactor, what percentage is converted to ethylene oxide?
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Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C;Hs(NO,),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. ? 2. Suppose 40.0 L of carbon dioxide gas are produced by this reaction, at a temperature of - 10.0 °C and pressure of exactly 1 atm. Calcuiate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits.
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Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H5(NO,),) into gaseous dinitrogen, gaseous O-0 dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 12.0 L of carbon dioxide gas are produced by this reaction, at a temperature of – 5.0 °C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Be sure your answer has the correct number of significant digits.
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6.A fuel is burned with 50% excess air and the combustion characteristics of the fuel oil are similar to C12H26. Determine the ff. a) air fuel ratio b) volumetric (molal) analysis of the products of combustion.
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H;(NO;),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 믐 x10 4C;H, (NO,), (1) → N, (3) + 0, (3) + CO,(8) + H,0(g) ? 2. Suppose 74.0L of carbon dioxide gas are produced by this reaction, at a temperature of - 13.0 °C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits.
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C3H5(NO3),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 52.0 L of carbon dioxide gas are produced by this reaction, at a temperature of-5.0 °C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Acces MacBook Air - F6 44 F7 1Il FO F.5 olo