1. A boiler burns fuel oil with the following analysis by mass : 80% C 18% H2 2%S 30% excess air is supplied to the process. Calculate the stoichiometric ratio by mass and the % Carbon Dioxide present in the dry products. (15.62/1 14.9% CO2) 2. A boiler burns coal with the following analysis by mass: 75% C 15% H2 7%S remainder ash Calculate the % Carbon Dioxide present in the dry products if 20% excess air is supplied. (16.5% CO2) 3. Calculate the % of each dry product when coal is burned stoichiometrically in air. The analysis of the coal is: 80% C 10% H2 5% S and 5% ash. (76.7%N, 22.5% CO2 0.8% SO2)

1. A boiler burns fuel oil with the following analysis by mass : 80% C 18% H2 2%S 30% excess air is supplied to the process. Calculate the stoichiometric ratio by mass and the % Carbon Dioxide present in the dry products. (15.62/1 14.9% CO2) 2. A boiler burns coal with the following analysis by mass: 75% C 15% H2 7%S remainder ash Calculate the % Carbon Dioxide present in the dry products if 20% excess air is supplied. (16.5% CO2) 3. Calculate the % of each dry product when coal is burned stoichiometrically in air. The analysis of the coal is: 80% C 10% H2 5% S and 5% ash. (76.7%N, 22.5% CO2 0.8% SO2)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

See similar textbooks

Similar questions

Methane (CH4) is burned with air (79% N2 and 21% O2 by volume) at atmospheric pressure. The molar analysis of the flue gas yields CO, %3D 10.00%, O2 = 2.41%, C0= 0.52%, and N2 = 87.07%. Balance the combustion %3D equation and determine the mass air-fuel ratio, the of stoichiomet- percentage ric air, and the of excess air. percentage
5. Reaction Enthalpy. balance and calculate AHa for the following chemical equations. AH (kJ/mol): HCN = 130.5, Cas(PO4)2=-4120.8, H3PO4--1288, SiCl₁=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl=-167.16 c) SICIL(1)+H₂O() SIO₂ (s) + нск HCl(aq)
Methanol is known to be the simplest alcohol, and is used as an antifreeze agent, a solvent, a fuel anda denaturant for ethyl alcohol. It is also known as “wood spirit”, as it is obtained from the pyrolysis ofwood. Methanol burns in air to produce CO2(g) and H2O(l). The chemical reaction is: 2CH3OH (ℓ)+ 3O2 (g) à 2CO2 (g) + 4H2O (ℓ)Calculate the enthalpy change for the reaction using the standard enthalpies of formation are found onthe chart provided.
How to find Moles of magnesium chloride. #7? Freezing-point depression constant (°C/m) Freezing-point of DI water (°C) Magnesium chloride Molar mass (g/mol) Mass of calorimeter (g) Volume of DI water (mL) Mass of magnesium chloride (g) Moles of magnesium chloride (mol) Mass of calorimeter + solution (g) Mass of calorimeter + solution + ice (g) Freezing-point of solution (°C) Mass of calorimeter + ice after decanting (g) Mass of ice added (g) Mass of ice remaining after decanting (g) Mass of melted ice (g) Mass of water in final solution (g) Mass of water in final solution (ko) Solution 1 MgCl2 95.21 17.28 49.0 1.46 0.0153 67.51 113.17 -1.02 43.92 45.66 26.64 19.02 67.79 0.06779 17.46 51.0 Solution 2 MgCl 95.21 2.11 0.0222 70.49 115.77 -1.46 1.86 41.32 45.28 23.86 21.42 72.34 0.07234 0.20 Solution 3 MgCl2 95.21 17.41 49.5 2.98 I
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?
5. Reaction Enthalpy. and calculate AH for the following chemical equations. AH (kJ/mol): HCN = 130.5, Cas(PO4)2=-4120.8, H3PO4--1288, SiCl=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl--167.16 b) Ca₂(PO4)2(s) + H₂SO4(0)- 0 CaSO4(s) + H3PO4(1)
- = T C 54°F Humid % Explanation O CHEMICAL REACTIONS Percent yield of chemical reactions 2 W |HC|HL| (@F11218HCHIHUSI https://www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IBMBkpcnaFu0F7Uj... FAX S Check بهر 3 * E $ X Gaseous ethane (CH₂CH3) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). If 0.469 g of water is produced from the reaction of 0.90 g of ethane and 5.2 g of oxygen gas, calculate the percent yield of water. Round your answer to 2 significant figures. 4 0 d R DE C Ś 96 % 5 T 6 G H "4+ & 7 B N U 144 * 00 C | 141 | a A 8 1 D-II ( 9 r K M || a ✓ DDI O s ) B Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | | O F ▬▬▬▬▬▬ fo 1 11² a P MC - MC insert C + 3/5 = prt sc } ♡ 4 Privacy Center Privacy Center | Acces 1 0 Chisom Seve E d 11:10 10/22/20
A steady-state process to recover crystalline potassium chromate (K,CrOz) from an aqueous solution of this salt is required. Four thousand kilograms per hour of a solution that is one-third K,CrO, by mass is joined by a recycle stream containing 36.4% K2CrO7, and the combined stream is fed into an evaporator. The concentrated stream leaving the evaporator contains 49.4% K,CrO; this stream is fed into a crystallizer in which it is cooled (causing crystals of K,CrO, to come out of solution) and then filtered. The filter cake consists of K,CrO, crystals and a solution that contains 36.4% K,CrO, by mass; the crystals account for 95% of the total mass of the filter cake. The solution that passes through the filter, also 36.4% K,CrO,, is the recycle stream. 1- Draw the flowchart of the system and put all known information. 2- Calculate the rate of evaporation, the rate of production of crystalline K,CrO7, the feed rates that the evaporator and the crystallizer must be designed to handle, and…
Solid baking soda (soolim bicarboncte) reacts with vinegar to groowee carbon dibxrde, water and sodium acetate (agueous). Hqueous lead (1D nitrate rea cts with potasesium sulfide (aqueous to produce a greciprtate of lead () sulfide and agueoos potasslum nitrode . * All equations must be balaned ŷ state symbole must be Activity included of symbols
Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.
The percentage composition of a liquid fuel by mass is, C = 86%, and H₂ = 11.75%, O₂ = 2.25% Calculate (i) the mass of air needed for the combustion of per kg of fuel; (ii) the mass of the products of combustion if 15% excess air is supplied.
5. Reaction Enthalpy. balance and calculate AHxn for the following chemical equations. AH (kJ/mol): HCN= 130.5, Ca3(PO4)2=-4120.8, H3PO4--1288, SiCl4=-640.1, SiO2= -910.9, Mg0=-601.6, HCl--167.16 a)NH₂(g) + O₂(g) + CH CH4(g) b)Ca₂(PO4)2(6) +H₂SO4(1) c)SICI(1) + H₂0 (1) d) MgO(s)+ H₂ H₂O(g) SIO₂ (s) + HCN HCN(g) + Caso (s) + H₂PO.(1) Mg(OH)2(s) H₂O(g) HCl(aq)