used in the manufacture of cement:ate rock (limestone) is heated to produce the quicklime, i.e., calcium oxide,Carbon dioxide is also released into the atmosphere when calcium carbon-PROBLEM 44CACO3(s)CaO(s) + CO;(g)Calculate the mass, in metric tons, of CO2 released per metric ton of lime-une used in this process. What is the mass of carbon that the air gains foreachof carbon dioxide that enters the atmosphere? Note that at leastgramos much carbon dioxide is released from combustion of the fossil fuel neededto heat the limestone as is released from the limestone itself.

This is an decomposition reaction.

Calculate the mass, in metric tons, of CO2 released per metric ton of lime- vane used in this process. What is the mass of carbon that the air gains for each gram of carbon dioxide that enters the atmosphere? Note that at least os much carbon dioxide is released from combustion of the fossil fuel needed to heat the limestone as is released from the limestone itself.

Calculate the mass, in metric tons, of CO2 released per metric ton of lime- vane used in this process. What is the mass of carbon that the air gains for each gram of carbon dioxide that enters the atmosphere? Note that at least os much carbon dioxide is released from combustion of the fossil fuel needed to heat the limestone as is released from the limestone itself.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 67QAP: When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and...

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
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?
Q2: A fuel oil is burned with 65% excess air, and the combustion characteristics of thefuel oil are similar to a paraffin series dodecane C12H26. Determine: (a) the actualair/fuel ratio (A/F) on a mole basis, (b) the actual air/fuel ratio (A/F) on a mass basis,and (c) the actual volumetric (molar) analysis of the products of combustion. State allthe assumptions that you would made before solving this question. Air contains 21%O2 and 79% N2 by mole. Do not solve in tabulated form.
Methane is produced in the human gut during digestion. As it passes through the digestive tract, it collects at thelower end and is emitted as flatulence. About 10% of a fart is composed of methane.__CH4 + __O2 → __ CO2 + __H2Oa) The average human fart contains 0.00643g of methane gas. Ifyou were to light said fart (and you SHOULD NOT), what mass ofoxygen would combust along with it?b) People, on average, pass 0.75L of gas per day. This is about0.0536g of methane per 24 hour period (remember, only ~10% ismethane). What mass of water could be generated by one personigniting their “methane emission”? c) How many water molecules is this? (SHOW ALL WORK IN TRAIN TRACKS)
Emissions from the burning of fossil fuels are often reported as gigatons ( Gt ) of carbon. In a calendar year, China emitted 2.9 Gt of carbon while the Unites States released 1.5 Gt of carbon. To what mass in gigatons of CO2CO2 do these amounts of carbon correspond?
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.
One of the sources of iron is magnetite, Fe3O4 (FeO and Fe2O3 mixed), which reacts with coke (carbon) to produce iron in the liquid state and carbon monoxide. If we assume that coke is pure carbon, how much is supplied to produce 10,000 metric tons of iron?
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)?
For the reaction C2H4 + 3O2 ---> 2CO2 + 2H2O, does this mean that ten (10) grams of CO2 produced reuired 0.345 mol O2?
For the following reaction: 5Ca + V2O5 --> 5CaO + 2V In one process 5 moñ of V2O5 react with 3 mol of acá. Calculate the theoretical yield of V in the unit of mol.
Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. Determine whether the data given confirm the formula of the hydrate. You must show any relevant calculation

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