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Part H Calculate the grams of H20 that would be produced. Express your answer with the appropriate units. HA ? m(H2O) = Value Units

Part H Calculate the grams of H20 that would be produced. Express your answer with the appropriate units. HA ? m(H2O) = Value Units

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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moles of CO2 formed = 31.0 g O2 × 1 mól 02 32.00 g 2 mol CO2 = 0.646 mol of CO2 produ 3 mol 02 Since the number of moles produced by O2 is less, it must be the limiting reagent. Part H Calculate the grams of H2O that would be produced. Express your answer with the appropriate units. ? m(H2O) = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Start by determining the limiting reagent (Part G), and then use the mass of this reagent to find the mass of product. When given a mass of reagent and asked to find the mass of product formed, start by converting the mass to moles using the molar mass of the reageit in g/mol. Once you have the number of moles of reagent, use the balanced chemical equation to find the number of moles of product formed. Finally, convert the moles of product formed to a mass using its molar mass. Next > vide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |
Transcribed Image Text:moles of CO2 formed = 31.0 g O2 × 1 mól 02 32.00 g 2 mol CO2 = 0.646 mol of CO2 produ 3 mol 02 Since the number of moles produced by O2 is less, it must be the limiting reagent. Part H Calculate the grams of H2O that would be produced. Express your answer with the appropriate units. ? m(H2O) = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Start by determining the limiting reagent (Part G), and then use the mass of this reagent to find the mass of product. When given a mass of reagent and asked to find the mass of product formed, start by converting the mass to moles using the molar mass of the reageit in g/mol. Once you have the number of moles of reagent, use the balanced chemical equation to find the number of moles of product formed. Finally, convert the moles of product formed to a mass using its molar mass. Next > vide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |
E Course Home Review I Constants I Periodic Table Part G Determine the limiting reactant, given 31.0 g of each reactant, in the following: C,HeO(1) + 302 (g) → 2CO2(g) + 3H2O(g) O H20 O C,H6O O 02 CO2 Submit Previous Answers Correct Use the 31.0g of each reactant and calculate the amount of product formed by each reactant to find the limiting reactant. If the comparison, then 1 mol C2H60 46.07g 2 Hol CO2 moles of CO2 formed 31.0 g C2H6O x = 1.35 mol of CO2 pro 1 pmol C2HO 1 mol 02 32.00 g 2 Hol CO2 moles of CO2 formed = 31.0 g'O2 x = 0.646 mol of CO2 produ 3 paol O2 Since the number of moles produced by O2 is less, it must be the limiting reagent.
Transcribed Image Text:E Course Home Review I Constants I Periodic Table Part G Determine the limiting reactant, given 31.0 g of each reactant, in the following: C,HeO(1) + 302 (g) → 2CO2(g) + 3H2O(g) O H20 O C,H6O O 02 CO2 Submit Previous Answers Correct Use the 31.0g of each reactant and calculate the amount of product formed by each reactant to find the limiting reactant. If the comparison, then 1 mol C2H60 46.07g 2 Hol CO2 moles of CO2 formed 31.0 g C2H6O x = 1.35 mol of CO2 pro 1 pmol C2HO 1 mol 02 32.00 g 2 Hol CO2 moles of CO2 formed = 31.0 g'O2 x = 0.646 mol of CO2 produ 3 paol O2 Since the number of moles produced by O2 is less, it must be the limiting reagent.
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