OSOPart 2SIO2Cr2O3CrHow many grams of the excess reactant are left after the reaction is complete?g1st attempt21 OF 23 QUESTIONS COMPLETED< 18/22 >+ VIEW SOLUTI The reaction of Cr₂O3 with silicon metal at high temperatures will make chromium metal.2Cr₂O₂ (s) +3Si(s)4Cr(1) +3SiO₂ (s)The reaction is begun with 170.00 g of Si and 118.00 g of Cr₂O3✓ 2nd attempt1Part 1Select the limiting reactant.Choose one or more:SISIO₂Cr2O3CrSee page 113hd See Periodic Table

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Answered: How many grams of the excess reactant…

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Chemistry

How many grams of the excess reactant are left after the reaction is complete? 8

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 6ALQ

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| Log In Q Englis 6 Self-Se G Gramn Tn Cours G traduc Build a C How M Co x G Eleme Balanc Parapl ge.com/course.html?courseld%=17244391&0penVellumHMAC=c6d3335eldc533558bc46d6c41bbfdf9#10001 E Reading list + Stoichiometry Review | Constants | Periodic Table raLA How many O2 molecules are needed to react with 6.73 g of S? Elemental S reacts with O2 to form SO3 according to the reaction Express your answer numerically in units of molecules. 25 + 302-2S0, > View Available Hint(s) as depicted here (Figure 1) 0.210 molecules Submit Previous Answers Figure X Incorrect; Try Again; 5 attempts remaining The value entered is the number of moles of S in 6.73 g. You need to find the number of molecules of O, needed to react with 6.73 g of S. 1 of 1 You may want to review Hint 4How to convert moles to moleciules Part B Oxygen Sulfur What is the theoretical yield of SO, produced by 6.73 g of S? Express your answer numerically in grams. Pearson O vA 3:48
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g In P Englis 9 Self Se G Gramn Tn Course G traduc * Balanc * Parap 4 Build a C How M G om/course.html?courseld%3D17244391&OpenVellumHMAC%=D9815e7584135fc006cabedb9aa0dda22#10001 The balanced reaction for the combustion of ethane is shown in the table. You allow 32 mol of ethane (CH6) to react with 4.1 mol oxygen (02). may be done using the Simulation, to indicate the amounts of all chemical species for the initial, change, and final conditions. Drag the appropriate amounts to their respective targets. • View Available Hint(s) Reset Help 2.3 mol 1.2 mol 0.0 mol 4.1 mol 2.0 mol 6.4 mol 3.2 mol 3.5 mol 11.2 mol 9.6 mol 2C,H.(g) + 7O2(g) → 4CO2(g) + 6H2O(g) Initial Change- Final Pearson Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | C
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PART V The empirical formula of an organic compound can be determined via combustion analysis. A typical combustion apparatus is shown below: loq Doy excess O₂ is added ofyll H₂O is trapped here 0 000 UDS sample is heated until it decomposes gainisicos tolesd Im 001 00 0 0 00 00 000 ITAAS CO₂ is trapped here A sample of the chemical is burned in oxygen in a tube packed with copper oxide to ensure complete combustion. The carbon in the compound is converted to CO2, which is absorbed in a tube packed with ascarite. The hydrogen is converted to water vapor and is absorbed in tube packed with drierite. The increase in weight of the absorber tubes corresponds to the CO2 and H₂O produced during combustion. Compounds X and Y do NOT contain any nitrogen, sulfur, or halogen atoms; both compounds do contain oxygen. A 1.0542 g sample of X was burned in a combustion apparatus. The results were: 75.2382 g 76.8377 g 81.4128 g Weight of ascarite tube before combustion Weight of ascarite tube after…