Part D-Yield Calculations Which of the following errors could cause your percent yield to be falsely high, or even over 100%? Select ALL that apply. Taking the mass of all samples with the lid included. Handling the crucible directly with your hands. Taking the mass of the empty crucible without the lid, but including the lid in all other mass measurements. Heating the sample too vigorously. Failing to completely decompose the sodium bicarbonate sample. Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining

Part D-Yield Calculations Which of the following errors could cause your percent yield to be falsely high, or even over 100%? Select ALL that apply. Taking the mass of all samples with the lid included. Handling the crucible directly with your hands. Taking the mass of the empty crucible without the lid, but including the lid in all other mass measurements. Heating the sample too vigorously. Failing to completely decompose the sodium bicarbonate sample. Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining

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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Use the References to access important values if needed for this question. Determine the molecular and empirical formulas for the substance shown in the ball-and-stick model below. C = black H=gray Molecular Formula In progress Empirical Formula Submit Answer Retry Entire Group 3 more group attempts remaining Previous Email Instructo Cengage Learning | Cengage Technical Support Q Search Bing %24 % & 5 7 8. R Y U F.
Chemistry Question 4 of 10 View Policies Show Attempt History Current Attempt in Progress Your answer is partially correct. Calculate the percent composition by mass for Fe(NO3)3. Use the molecular weights to two decimal places in your calculations. a) %Fe - 23.09 b) %N-i 5.718 c)%0- 19.83 eTextbook and Media Hint Save for Later Attempts: 5 of 10 u
y Cour o T Macmilla X Back b/ui/evo/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883& Course M X = v Submit Answer Section A compound is found to contain 11.21 % hydrogen and 88.79 % oxygen by mass. What is the empirical formula for this compound? To answer the question, enter the elements in the order presented above. 9. Percent Composition to Empirical Formula: This is group attempt 1 of 10 References Use the References to access important values if needed for this question. A- HOMEW 0 A compound is found to contain 37.23 % carbon, 7.827 % hydrogen, and 54.94 % chlorine by mass. What is the empirical formula for this compound? To answer the question, enter the elements in the order presented above. Mind Autosaved at 5:51 PM
Mole Ratio Worksheet All the following chemical reactions are balanced, please write your mole ratios like this 1:2, and ½ both ways. This is important in the future. Here’s a video in case you need help, or missed the lecture notes, lecture, and practice problems. https://www.youtube.com/watch?v=c9beXPzJ-Fs Step 1) RTFQ- read the funny question, circle the known (what I know), and what you need (what I want to know). Step 2) Set up DA, your KNOWN in the top left box, then cancel the units till you get the unit you want. Step 3) Do the math= calculate __Zn + 2HCl __ZnCl2 + __H2 balanced equation.a. How many moles of hydrogen are produced from the reaction of three moles of zinc? 1.Mole to mole prob, therefore set up mole ratio 2.Set up DA______________= 3.math How many moles zinc are needed to produce 3.5 moles of zinc chloride? Mole to mole prob, therefore set up mole ratio 1.Mole to mole prob, therefore set up mole ratio 2.Set up DA______________= 3.math How…
What mass of magnesium chloride is produced from the single replacement reaction of 6.45 moles of hydrochloric acid and magnesium? Answer: number unit of formula 80 F3 Answer: [Select] [Select] *For chemical formulas: enter subscripts as normal number, and no spaces. ◄ Previous $ 4 JAN 24 Q F4 % 5 O F5 6 1 tv mol F6 & 7 8 F7 10 * 8 DII F8 A ( Next ▸ of 9 DD F9
SIMULATION Compounds and Moles DO Mass: 6.00 g H₂O SO₂ 64.058 Ru(CO) 5 241.12 SF6 146.05 88.004 207.29 CF4 OXEF4 XeF4 Xe Molar Mass 18.015 F Mass (g) 6.00 3.80 2.20 What is the ratio Recheck Percent Compositions 88.81 O 49.95 O 24.90 C 33.17 O 5th attempt 11.18 H 50.04 S 41.91 Ru 21.95 S 13.64 C 63.34 Xe Amount (mol) 0.0289 0.0289 0.116 Enter your answer as an integer. 78.04 F Next (13 of 15) 86.35 F 36.35 F amount (mol) F atoms ? amount (mol) Xe atoms Particles 1.74 x 1022 1.74 x 1022 6.97 × 1022 X
If a student records a percentage yield of more than 100%, what are the possible errors? Select all that apply O not washing the product well enough thereby comtaminating the product with other side products formed during the reaction. incomplete reaction that led to loss of product loss of product during a separation process in the experiment O not completely drying the product before weighing the actual yield.
B. Formula of a Hydrate 23.43 29.24 26.31 26.28 1. Mass of crucible 2. Mass of crucible and hydrate 3. Mass of crucible and anhydrate 3a. Mass of crucible and anhydrate (second heating) Calculations 4. Mass of hydrate 5. Mass of anhydrate 6. Mass of water lost
THIS Webpage is using significant memory. Closing it may improve the responsiveness of your Mac. < Adaptive Chapter 8 A li 47% 画04/11/21 mmorr197@students.kennesa SCORE Full Adaptive O KNEWTON POWERED BY Learning Objectives Mastery " 1 2 2 Learning Objective: 8.C Quantify mass and number of moles in solutions given their concentrations. Adaptive Assignment e See page 336 Question 1st attempt i See Periodic Table O See Hint A concentrated solution of HF has a molarity of 9.75 M. You add 31.00 mL to a flask and then dilute with water. The mass of the final solution is 125.0 g. What is the mass percent of HF? % < 12 * SUBMIT ANSWER MacBook Air 888 DD $10 F3 F2 F4 F5 F6 F7 FB F9
Answer letter D, E and F only. ll. Direction: Carefully read the following problemsDo the following :A. Balance the chemical equation B. Identify the limiting reactant and the excess reactant if applicable;C. Compute for the theoretical yield;D. Determine the percentage yield of the reaction;E. Calculate the percent error andF. Compute for the excess amount of the excess reactant if applicable;
MISSED THIS? Watch KCV Limiting Beactant. Theoretical Yield and Percent Yield WE Limiting Reactant and Theoretical Yield Read Section 4.4. You can click on the Review link to access the section in your eText Find the limiting reactant for each initial amount of reactants 2Na(s) + Bra(g)-> 2NaBr(s) Part A 7 mol Na and 3 mol Bry Express your answer as a chemical formula. View Available Hint(s) Hint 1. Identify conversion factors between the numbers of moles of Na and NaBr and between the numbers of moles of Bry and NaBr ΑΣΦΑ ?
Name:Tashina & 3-28-22 Period: Stoichiometry - Mole to Mole Ratio **Success Criteria: I can calculate the weight of molecules if given the number of molecules or vice versa. Directions: Solve the following mole ratio problems. 1. N +_3 _H,→ 2_NH, How many moles of Hydrogen are needed to completely react with two moles of Nitrogen? 2. Co KCIO, → C6 КСІ + 9 02 How many moles of Oxygen are produced by the decomposition of six moles of Potassium Chlorate? a moles 02 3. Zn + HCl → ZnCl, + H2 How many moles of Hydrogen are produced from the reaction of three moles of Zinc with an excess of Hydrochloric Acid? 4. C;Hg + O2 CO3 + H,0 How many moles of Oxygen are necessary to react completely with four moles of Propane (C;Hs)? 5. KĄPO, + Al(NO;); KNO, + AIPO4 How many moles of Potassium Nitrate are produced when two moles of Potassium Phosphate react with two moles of Aluminum Nitrate? Cu + AGNO, - Cu(NO3)2 + Ag BONUS: a. How many moles of Cu are needed to react with 3.50 moles of AgNO,? b. If…