Use the following atomic weights and quantities to calculate the overall % yield of benzopinacol. Remember that your yield must be based on the stoichiometry (balance theequation!), the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding theanswer is a whole number, do not include a decimal point.C = 12, H = 1, O = 16benzophenone isopropanol acetic acid→>> benzopinacolformulaformula weightmilliliters2.0930.889density0.7861.05gramsmoles38.1034.214Answer:% yield?

% yield of Benzopinacole is 10.13 % Explanation: Mass Benzophenone = 38.103 gMass of Isopropanol…

Answered: Use the following atomic weights and…

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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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")
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Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 59.8 grams N2 in the presence of excess H2 gas according to the following balanced chemical equation: N2(g) + H2(g) → NH3(g) X TING AMOUNT ADD FACTOR ANSWER RESET *( ) 17.04 3.52 1.01 14.01 59.8 3 4.27 8.54 72.7 2.13 28.02 145 1 7.04 g/mol N2 g N2 g/mol NH3 mol NH3 mol N2 g NH3
Consider the following chemical reaction HCl (aq) + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3 Determine the excess reactant The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction Determine the type of this chemical reaction
If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of oxygen gas are also given off. Find the percent yields. - 2 KCIO3 → 2 KCI + 3 02 Please remember significant figures in your answer! Units not required.
Can you please help me with question 1.
Use the following atomic weights and quantities to calculate the overall % yield of benzil. Remember that your yield must be based on the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C = 12, H = 1, Cu = 63.5, N = 14, O= 16 formula formula weight grams moles Answer: benzoin+ammonium nitrate + copper(II) acetate benzil 37.264 3.565 14.006 % yield 6.644
A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.19 L) 1 mL 10-³ 146.86 g mol 1.04 mL = ☐ x10 ロ･ロ X I 00
Calculate the theoretical mass and the percent yield. Please show all work!
Use the following atomic weights and quantities to calculate the overall % yield of caprolactam. Remember that your yield must be based on the stoichiometry, the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C = 12, H = 1, N = 14, O = 16, P = 31 formula formula weight milliliters density grams moles Answer: 85% phosphoric acid cyclohexanone oxime 22.802 1.7 4.446 % yield caprolactam 4.179 ?
*Please show all your work for this question using Dimensional Analysis. Titanium Dioxide (TiO2) is an industrial chemical used as a white pigment in paint. The conversion of volatile TiCl4 to TiO2 occurs according to the following reaction: 1 TiCl4(g) + 1 O2(g) --> 1 TiO2(g) + 2 Cl2(g) Using the above reaction, calculate the percent yield of Cl2 if 19.2 g TiCl4 reacts with an excess oxygen to give an actual yield of 11.1 g Cl2. Round your answer to the tenth's (0.1) place.
[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.

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