A fuel oil is analyzed and found to contain 85.0 wt% carbon, 12.0% elemental hydrogen (H), 1.7% sulfur, and the remainder noncombustible matter. The oil is burned with 20.0% excess air, based on complete combustion of the carbon to CO2, the hydrogen to H2O, and the sulfur to SO2. The oil is burned completely, but 8% of the carbon forms CO. Calculate the molar composition of the stack gas.
Trending nowThis is a popular solution!
Chapter 4 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
Additional Science Textbook Solutions
Process Dynamics and Control, 4e
Elements of Chemical Reaction Engineering (5th Edition) (Prentice Hall International Series in the Physical and Chemical Engineering Sciences)
Foundation Design: Principles and Practices (3rd Edition)
Electrical Engineering: Principles & Applications (7th Edition)
Introductory Circuit Analysis (13th Edition)
Automotive Technology: Principles, Diagnosis, And Service (6th Edition) (halderman Automotive Series)
- Calculate the grams of CO2 produced in the complete combustion of a 406-g bottled gas that consists of 72.7 wt% propane (C3H8) and 27.3 wt% butane (C4H10). Use C = 12.01 g/mol; H = 1.01 g/mol; O = 16.00 g/mol.arrow_forwardA fuel containing 80% CH4 and 20% C2H6 is burned with dry air. Sixty percent of the carbon burned goes to CO2, the rest going to CO. Fifty percent excess air is used. Calculate the number of moles of each constituents of the wet flue gas produced by combustion of 100 mole of fuel gas, and also the Orsat analysis of the flue gas.arrow_forwardA gaseous fuel contains by volume:CO2 = 2.6 % ,CO = 6 %, O2= O.6 % ,N2= 3.66 % ,H2= 48.0%CH4= 34 %, C2H4=5.2 %Calculate the minimum volume of air required for complete combustion of 100 m3 of the gas. If 50 % excess air is supplied, find the volume of each of the dry constituents of the flue gas.arrow_forward
- What is the mole ratio for O2 gas to water for the balanced equation for the complete combustion of butane. 2C4H10(g)+ 13O2(g)-> 10H2O(g) + 8CO2(g)arrow_forwardA sample containing a mixture of SrCl, · 6 H,0 (MW = 266.62 g/mol) and CSCI (MW = 168.36 g/mol) originally weighs 1.6017 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl, · 6 H,0, leaving the anhydrous SrCl,. After cooling the sample in a desiccator, it has a mass of 1.1433 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 320 °C SrCl, · 6 H,0(s)- SrCl, (s) + 6 H,O(g) wt% Sr = wt% Cs = wt% CI =arrow_forwardThe oxidation of ethylene to produce ethylene oxide proceeds according to the equation2C 2H 4 +O 2 → 2C 2H 4O The feed to a reactor contains 100 kmol C 2H 4 and 100 kmol O 2. If the reaction proceeds to a point where 60 kmol of O 2 is left, what is the fractional conversion of C 2H 4? The fractional conversion of O 2? The extent of reaction?arrow_forward
- When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 35.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3 Submit = Part B 0 370.8 HÅ atm Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10 (9) + 1302 (g)→8CO2 (g) + 10H₂O (1) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 2.20 g of butane? Express your answer with the appropriate units.arrow_forwardHydrogen gas has the potential for use as a clean fuel inreaction with oxygen. The relevant reaction is2 H2(g) + O2(g) ---->2 H2O(l)Consider two possible ways of utilizing this reaction asan electrical energy source: (i) Hydrogen and oxygengases are combusted and used to drive a generator, muchas coal is currently used in the electric power industry;(ii) hydrogen and oxygen gases are used to generate electricitydirectly by using fuel cells that operate at 85 °C.(a) Calculate ΔH° and ΔS° forthe reaction. We will assume that these values do notchange appreciably with temperature. (b) Based on thevalues from part (a), what trend would you expect forthe magnitude of ΔG for the reaction as the temperatureincreases? (c) What is the significance of the change inthe magnitude of ΔG with temperature with respect to the utility of hydrogen as a fuel? (d) Based on the analysishere, would it be more efficient to use the combustionmethod or the fuel-cell method to generate electricalenergy from…arrow_forward8. A hydrocarbon fuel is fully combusted with 495.97 g of oxygen to yield 880.2 g of carbon dioxide and 396.34 g of water. A.) Find the empirical formula for the hydrocarbon. B.) The molecular formula of the hydrocarbon if its MW is 142.29 g/mol. 9. (5 points) The K, value of the reaction N₂O4 2NO₁₂ (g) ²(g) is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23 atm while NO₂ is 0.750 atm? Is the process spontaneous? 10. (5 points) The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C. Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit J/K.arrow_forward
- A coal sample having the following composition: C = 80%, H = 4%, O = 3%, S = 2%, N = 3%, ash = 5% and moisture = 3%. Calculate the quantity of air needed for the complete combustion of 1 kg of coal, if 60% excess air is supplied. %3Darrow_forwardPhotosynthesis in plants converts carbon dioxide and water into glucose (C6H1206) and oxygen according to the equation below. 6CO2 (g) + 6H20a → C6H1206 (s) + 602 (g) Substance СО2 (8) H20M C6H1206 (s) 02 (g) kJ AH°; (mol -393.5 -285.8 -1273.3 J H° mol. k 213.6 69.9 209.2 205.0 Calculate the AHº, ASº, and AGº. Is the reaction spontaneous at standard conditions?arrow_forwardb) Calculate the stoichiometric fuel/air mass ratio and product gas composition for the combustion of Hexane in air. (C=12, H=1, O=16, N=14)arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY