Rev MISSED THIS? Read Section 4.4 (Pages 149 - 155); Watch KCV 4.4, IWE 4.6. Correct answer is shown. Your answer 233.2 kg was either rounded differently significant figures than required for this part. Important: If you use this answer in later parts, use the full unrounded value in y The theoretical yield is the mass of product that could hypothetically be produce- determine the theoretical yield of urea (CH N20), convert the molar amount of reactant (NH3) as determined in Part A to kilograms (kg). Use the molar mass moles (mol) to grams (g). Then, convert grams to kilograms using the convers Urea (CH,N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH) with carbon dioxide as follows: 2NH3(aq) + CO2(aq) CH N20(aq) + H20(1) In an industrial synthesis of urea, a chemist combines 132.1 kg of ammonia with 211.4 kg of carbon dioxide and obtains 163.8 kg of urea. 60.06 g CH,N,O 1 mol CH N,O 1 kg 3880.7 mol CH,N20 x 1000 g Part C Determine the percent yield for the reaction. Express your answer using three significant figures. » View Available Hint(s) Submit

Rev MISSED THIS? Read Section 4.4 (Pages 149 - 155); Watch KCV 4.4, IWE 4.6. Correct answer is shown. Your answer 233.2 kg was either rounded differently significant figures than required for this part. Important: If you use this answer in later parts, use the full unrounded value in y The theoretical yield is the mass of product that could hypothetically be produce- determine the theoretical yield of urea (CH N20), convert the molar amount of reactant (NH3) as determined in Part A to kilograms (kg). Use the molar mass moles (mol) to grams (g). Then, convert grams to kilograms using the convers Urea (CH,N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH) with carbon dioxide as follows: 2NH3(aq) + CO2(aq) CH N20(aq) + H20(1) In an industrial synthesis of urea, a chemist combines 132.1 kg of ammonia with 211.4 kg of carbon dioxide and obtains 163.8 kg of urea. 60.06 g CH,N,O 1 mol CH N,O 1 kg 3880.7 mol CH,N20 x 1000 g Part C Determine the percent yield for the reaction. Express your answer using three significant figures. » View Available Hint(s) Submit

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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Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, from the complete reaction of 59.8 grams N, in the presence of excess H, gas according to the following balanced chemical equation: 3 H,(g) - 2 NH,(g) RTING AMOUNT ADD FACTOR ANSWER RESET *( ) 72 7 1.01 50 0 17 04 29 02 145 4 27
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Product Composition and Reaction Stoichiometry Suppose SH2 and O2 react to produce H20, and a sulfur oxide which contains 40.05% sulfur by mass. Complete the reaction equation by entering the coefficients of the reactants and products and also the empirical formula of the sulfur oxide product. SH2 + H20 + All coefficients must be reduced to the smallest possible integers. Note that, while it is not usual to write coefficients of exactly 1, you must enter "1" in the response box, if that is the correct value. The formula for the sulfur oxide must be written with the S symbol first and O second. The usual subscription of numbers in the formula is to be inferred (e.g. the formula for water would be entered simply as "H2O")
1.) Convert both initial reactant values into moles. 2.) Which reagent is the limiting reagent? 3.) What mass of urea, CO(NH2)2, is produced? Urea has a molar mass of 60.1 g/mol.
When NaHCO3 completely decomposes, it can follow this balanced chemical equation: 2NaHCO3 → Na₂CO3 + H₂CO3 A. Determine the theoretical yields of each product using stoichiometry if the mass of the NaHCO3 sample is 3.24 grams. (Show work for both) B. In an actual decomposition of NaHCO3, the mass of one of the products was measured to be 2.01 grams. Identify which product this could be and justify your reasoning. C. Calculate the percent yield of the product identified in part B. (Show your work)
Gaseous methane (CH4) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). What is the theoretical yield of carbon dioxide formed from the reaction of 0.80 g of methane and 2.1 g of oxygen gas? Round your answer to 2 significant figures. THED X 5 ? Explanation Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DII DD J 4) F1 F8 F9 F10 F12 T 0 esc ! 1 @ 2 Check F2 #3 80 F3 S4 $ 000 000 F4 % 5 F5 MacBook Air F6 A 6 & 7 44 F7 * 00 8 ( 9 - F11 + 11 A alo Ar 00 dele
Dilution Problems, Chemistry, Molarity & Concentration Examples,... M O O CHEMICAL REACTIONS Reaction sequence stoichiometry In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe₂O3(s) + 3CO(g) → 2Fe(s) + 3 CO₂ (g) E crosoft O V Blast furnaces extra pure iron from the iron (III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C(s) + O₂(g) 2 CO (g) W Suppose the yield of the first step is 84.% and the yield of the second step is 63.%. Calculate the mass of oxygen required to make 3.0 kg of iron. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. G Microsoft Microsoft 6.52.210... Explanation BO C Check 9,269 x10 믐 103 X OCT 24 ロ・ロ átv 2 3/5 DOZA Simrat 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility W E ol Ar
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
Can someone help me out with the conversion aspect of this question? Im getting the answer right but the conversion wrong
Given a balance chemical equation , 2 C2H6 (g)+7 O2 (g) —> 4 CO 2 (g)+6 H2O(g) If reaction mixture contains 5 moles of O2 (g) with 6 moles of C2H6 (g) how many moles of CO2 will be produced? Hint: Identify the limiting reactant first Round and report your answer with a number having one decimal point. Enter that number into the answer box Don't include unit.
A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. M83N2 + 3H20 – 2NH3 + 3MgO The yield of Mgo is 3.99 g. What is the percent yield in the reaction? Atomic weights: Mg=24.31, N=14.01, H=1.01, O=15.99. Input values only with 2 decimal places.