ime's Up!A compound containing only carbon,hydrogen, and oxygen is analyzed usingcombustion analysis. When 46.3 g of thecompound is burned, 84.8 g of carbondioxide and 23.2 g of water are collected.1In order to determine the moles of carbonin the compound, first determine themoles of carbon dioxide that were47+/-produced from the combustion.Tap here or pull up for additional resourcesBT1F2BT2F3F4F5F6F7F82$%587IIS4#3

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A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 46.3 g of the compound is burned, 84.8 g of carbon dioxide and 23.2 g of water are collected. In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion.

A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 46.3 g of the compound is burned, 84.8 g of carbon dioxide and 23.2 g of water are collected. In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion.

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 52QAP: Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases...

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Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.
5. A test run using this coal showed a dry products of combustion analysis by volume of nitrogen equals 82.5%, molecular weight of 30 kg flue gas per mol dry flue gas, and the weight of this dry flue gas is 15.03 kg per kg of coal. The actual ash-pit sample was 0.15 kg per kg of coal, of which 20% was carbon. What is the percentage excess air supplied to the fuel combustion in percent? 6. Find the partial pressures in kPa of oxygen in atmospheric air of 100 kPa which contains by weight 23.1% oxygen and 76.9% nitrogen.
Leaming Calculate the number of pounds of CO, released into the atmosphere when a 13.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C,H,13, and that the density of gasoline is 0.692 g · mL-. This assumption ignores additives. Also, assume complete combustion. CO, released: lb - TOOLS x10
Blackboard Learn → C Gmail < app.101edu.co YouTube X STARTING AMOUNT Aktiv Chemistry Maps Welcome to MyTCC X W S #1 X E D X b Home | bartleby 403 Forbidden: Ac... ADD FACTOR x() 32.91 g CO₂ R Determine the mass in grams of CO₂ that are produced by the complete reaction of 10.49 grams of C«Hu (cyclohexane) according to the following combustion reaction: F 0.1246 44.01 mol CO₂ CH()+9 O:(g) 6 CO2(g) + 6 H₂O(g) → T V 5.486 g O₂ 84.16 X 6 G Question 45 of 50 18.02 g H₂O Your Sets | Quizlet Y 10.49 B 7 ASUS ANSWER 32.00 mol O₂ H 6 mol H.O 8 N J 1 9 X 1 RESET 2 9 C«Hu 6.022 x 10 Sign In or Sign Up | Chegg.cc X + Q☆ K M mol CH 15 O O 10 P @
Page < 2 of 2 ZOOM + 7. Write balanced chemical eqess | esc | to exitTO Screen ctions. a. production of ammonia, NH3(g), by combining N2(g) and H2(g) b. production of methanol, CH3OH(1), by combining H2(g) and CO(g) c. production of sulfuric acid by combining sulfur, oxygen, and water 8. Diborane and related compounds were proposed as rocket fuels in the 1950s. A representative reaction for this class of molecules is that of B2H6 and O2 to form B2O3 and H2O. Write the balanced chemical equation for this process. 9. Silicon nitride, Si3N4, is used as a reinforcing fiber in construction materials. It can be synthesized from silicon tetrachloride and ammonia. The other product is ammonium chloride. Write the balanced chemical reaction for this process. 10. Classify the following compounds as electrolytes or nonelectrolytes: a. potassium chloride, KCl b. hydrogen peroxide, H2O2 c. methane, CH4 d. barium nitrate, Ba(NO3)2
69. Methane is burned with oxygen to yield carbon dioxide and water. 150 kg-moles/hr of a stream consisting of 20 mole-% CH, 60 % O,, and 20 % CO,are fed into a reactor, in which a conversion of 90% of the limiting reactant is obtained. Calculate the molar composition (mole - %) of the product stream
✓ 个 < app.101edu.co STARTING AMOUNT X How many grams of oxygen gas are produced when 2.43 x 104 g of KCIO, are completely reacted according to the following chemical equation: 3.5 1 ADD FACTOR * ( ) 32.00 9.52 x 10-5 g KCIO3 2 KCIO3(s) → 1.90 x 10-4 Question 31 of 38 2 mol KCIO3 O 3 2 KCI(S) + 3 M 74.55 mol KCI ANSWER 31 1.98 x 10-6 5.95 x 10-6 mol O₂ O₂(g) 2.43 x 104 6.022 x 10²3 g 0₂ by RESET 2 2.97 x 10-6 122.55 g KCI Feb 23 7:11 O
A sample petrol on analysis gave C = 85% and H2 = 15%. Calculate the weight of air for complete combustion of 100 kg of petrol. What is the number of moles of air equivalent to this? MWair = 29.
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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 44 CACO3(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 for each of carbon dioxide that enters the atmosphere? Note that at least gram os much carbon dioxide is released from combustion of the fossil fuel needed to heat the limestone as is released from the limestone itself.
Water of Hydration Record the mass empty evaporating dish ( or crucible). Record the mass of dish before heating the hydrate 29.00g 31.11g Measure the mass of the dish and the anhydrous material here. 30.75g Determine the chemical formula of the original hydrate. Show your calculation here: Anhydrate: Cu3(PO4)2 Mass of anhydrate menm Moles of the anhydrate - Mass of water Moles of H20
Ise SEVENTH EDITION sented by Macmillan Leaning Calculate the number of pounds of CO, released into the atmosphere when a 13.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, CaH8, and that the density of gasoline is 0.692 g · mL1. This assumption ignores additives. Also, assume complete combustion. 600.54 CO, released: lb Incorrect

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