E ResultO GradesO CP RefeO Grades||Co ΧG A mixtu6 ModulM Roux Li6 Your SIM Inbox ( +bnc Your St& Cle 4envellum.ecollege.com/course.html?courseld%3D16985674&OpenVellumHMAC=Dd20f081859e6de97f65e31513d4bfdc9#10001I Review | Constants | PericConsider the following reaction:2SO2(g) + O2(g) → 2SO3(9)Part APart BWhat is the theoretical yield of SO3?nso,molSubmitPrevious Answers Request AnswerX Incorrect; Try Again; 5 attempts remainingPart CIf 181.9 mL of SO3 is collected (measured at 318 K and 50.8 mmHg ), what is the percent yield forreaction?P Pearsonto search74°F CloudyO O 4)

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M Review | Constants | Peric Consider the following reaction: 2SO2(g) + O2(9) → 2SO3(9) Part A Part B What is the theoretical yield of SO3? να ΑΣφ nso, mol Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part C If 181.9 mL of SO, is collected (measured at 318 K and 50.8 mmHg ). what is the percent yield fom reaction? P Pearson

M Review | Constants | Peric Consider the following reaction: 2SO2(g) + O2(9) → 2SO3(9) Part A Part B What is the theoretical yield of SO3? να ΑΣφ nso, mol Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part C If 181.9 mL of SO, is collected (measured at 318 K and 50.8 mmHg ). what is the percent yield fom reaction? P Pearson

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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shift How many moles of NO₂ would be produced from 8.4 mol of O₂ in the reaction below assuming the reaction has a 57.0% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g) tab Tap here or pull up for additional resources caps lock control ! 1 Q A Z 1 option @ 2 W S X # 出 cmd E D $ 4 C R F 5 V T G 6 Question 1 of 10 Y B & 7 H U N 8 J 1 M K < I ab 1 4 7 +/- L P 5 8 : L
I Review | Constants | Periodic Table The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Submit Previous Answers v Correct ?NH3(9)+?O2(9)–→?NO(g)+?H2O(g) Correct answer is shown. Your answer 443.34 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O2 needed to produce 18.0 mol of NO. However, in the industrial production of NO, oxygen is added in excess of this amount. Part B What volume of H20(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. • View Available Hint(s) volume of H20 = L
6. Hydrogen and iodine react to produce hydrogen iodide. If 3 moles hydrogen and 3 moles iodine react to produce 163 grams of hydrogen iodide, what is the percent yield? Assume constant temperature and pressure. The molar mass of H2 is 2.02 g/mol, of 12 is 253.8 g/mol, and of HI is 127.9 g/mol. H2(g) +12(g) → 2 HI(g)
mework X WP NWP Assessment Player Ul Appli x education.wiley.com/was/ui/v2/assessment-player/index.html?launchld=d7fbf299-2b78-4aab-9fe4-25d65ce73435#/question/4 cer 9 Homework tly sunny Question 5 of 6 View Policies Show Attempt History Current Attempt in Progress X Incorrect. What is the limiting reactant? H₂(g) + Cl₂(g) i. 50.0 How many grams of hydrogen chloride can be produced from 0.490 g of hydrogen and 50.0g chlorine? The balanced equation is: 17.9 2 Hint + 2 HCI(g) eTextbook and Media Save for Later g HCl 0/2 O Search 13 Attempts: 3 of 5 used Submit Answer
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We are determining the rate law equation for a reaction A + B + C → ABC in which a dramatic and instant color change tells us that reactants are used up and product is formed. (Concentrations used in all experiments are [A] = 2.0M, [B] = 1.0M and [C] = 3.0M) This is the data for questions 5 through 8: Volume of Volume of Volume of Volume of water, mL Time from mixing to dramatic color change, sec A, B, C, mL mL mL 0.5 2.0 2.0 95.5 36 1.0 2.0 2.0 95.0 6
Solid phosphorus (P) and chlorine (C1₂) gas react to form solid phosphorus pentachloride (PC15). Suppose you have 11.0 mol of P and 7.0 mol of Cl₂ in a reactor. Could half the P react? If you answered yes, calculate how many moles of PC15 would be produced after half the P was used up. Round your answer to the nearest 0.1 mol. yes no mol 0x x10 X Ś
TUTOR Percent Yield Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog: H2(g) + C¿H4(g) C,H6(g) If there is 16.1 g H, and excess C,H, present, the reaction yields 179 g C,H, Calculate the percent yield for the reaction Submit Show Approach Show Tutor Steps Submit Answer Try Another Version Show Hint 11:44 AM 3/5/2020 FLV O search hp home delete 80
7:27 O O @ X all 25% Submission Name: De Ocampo, Cyzvell N. Date: 11-30-21 Strand and Section: 12STEMA7 Teacher: Mr. Reynante S. Santos Homework 7.1| Stoichiometry in Chemical Reactions Directions: Use the balanced chemical equation to solve the following problems. 4Fe + 302 → 2FE203 1. How many moles of Fe,0z are produced when 7.27 grams of Fe is reacted? 1 mel Fe 2 mol Fe203 0.07 or 0.0650 mol Fe203 7.27 gFe 55.85 g Fe 4 mel Fe 2. How many moles of Fe,0, are produced when 19.0 grams of 0, is reacted? 1 mel02 2 Fe203 19:0 g02---- = 0.40 or 0.395 mol Fe203 32 g02 3 mele2 3. How many moles of 0, are needed to react with 25.9 grams of Fe? 1 met-Fe 3 mol 02 = 0.35 mol 02 25.9 Fe 55.85 g Fe 4 met Fe COMMENTS FILES (1) RUBRIC
2:24 Question 7 of 16 Consider the following reaction: 2 SO₂(g) + O₂(g) ⇒ 2 SO3(g). If you chamber, you would observe decrease the volume of the reaction A) an increase in SO2. B) an increase in O₂. C) an increase in SO3. D) both (A) and (B). E) none of the above. Submit Tap here or pull up for additional resources
11:11 AM Sun Oct 22 < Question 16 of 34 13% % Submit If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.0 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂(g) → 2 NO2 (g)