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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The number of moles of NaOH used is 0.5 and number of moles of methyl salicylate is 0.023 . What is the limiting reagent and please calculate the theoretical yield of the salicylic acid product in grams
Thank you for your explanation, I'm however confused by the multiplication of each. For example, the first one mentions x 3 to CuBr2 and x 2 to AlBr3, this process of cancelling out to create even moles is the balancing? I also wanted to know what the proper classification was for those three you answered? I felt like I had the first two wrong, I wasn't sure if they were single or double replacement.
How much aspirin can be made from 100.0 g of salicylic acid and 100.0 g of acetic anhydride? If 122 grams of aspirin are obtained by the reaction, what is the percent yield?C7H6O3 + C4H6O3 arrow C9H8O4 + HC2H3O2 salicylic acid acetic anhydride aspirin acetic acid
About 300 grams of glucose was fermented with 20 grams of yeast inside a fermenting vessel for 2 weeks. Calculate the percent yield of ethyl alcohol in mL or %(v/v) if the actual yield of the fermentation set-up is at 84.50 mL alcohol. Assume the density of ethanol is at 0.789 g/mL. C6H12O6 + H2O à 2C2H5OH + 2CO2 Molar Masses: Glucose: 180.156 g/mole; Ethanol: 46.07 g/mole Water: 18.00 g/mole Report your answers in two decimal places.
I was told to repost the full question because the items that were only answerd is a, b, and c so please answer only items d and e.Ethyl chloride (C2H5Cl) is formed by reacting ethylene (C2H4) with hydrogen chloride (HCl). a. Write the balanced chemical equation. b. If 30 g of ethylene react with 30 grams of hydrogen chloride, which of the two is the limiting reagent? The excess reagent? c. Calculate the theoretical yield of the limiting reagent. d. Determine the mass remained. e. If 43 g of ethyl chloride was formed, what is the percent yield?
1- An unknown compound has the following chemical formula: P2Ox where x stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 5.0mol of oxygen and 3.3mol of phosphorus. Write the complete chemical formula for the unknown compound. 2-Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. CH3CH2CH3 (g) + O2 (g) → CO2 (g) + H2O (g) 3-An aluminum atom has a mass of 4.48x 10-23 g and a small airplane has a mass of 5000.kg. Use this information to answer the question below. Be sure your answers have the correct number of significant digits. What is the mass of 1 mole of aluminum atoms? ____g 4- The chemical formula for propane is: CH3CH2CH3Calculate the molar mass of propane. Round your answer to 2 decimal places. ____ g ⋅ mol-1 5-An electrical engineer measures the frequency of a satellite radio transmission. The frequency is…
The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3)(NaHCO3) reacting with one mole of hydrochloric acid (HCl)(HCl) to produce one mole of carbonic acid (H2CO3),(H2CO3), and one mole of sodium chloride (NaCl).(NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 22 mol NaHCO3NaHCO3 and 88 mol HCl.HCl. moles of carbonic acid : mol Which of the two reactants limits the number of moles of H2CO3H2CO3 that can be made? HClHCl NaHCO3NaHCO3 How much excess reactant remains after the reaction? excess reactant : mol
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Butane, C4H10C4H10, reacts with oxygen, O2O2, to form water, H2OH2O, and carbon dioxide, CO2CO2, as shown in the following chemical equation: 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. Also, notice that the coefficient for butane (2) is one-fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth the number of moles of carbon dioxide that you produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. What is the molar mass of butane, C4H10C4H10? Express your answer to four significant figures and include the appropriate units.
Butane, C4H10C4H10, reacts with oxygen, O2O2, to form water, H2OH2O, and carbon dioxide, CO2CO2, as shown in the following chemical equation: 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. Also, notice that the coefficient for butane (2) is one-fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth the number of moles of carbon dioxide that you produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. Calculate the mass of water produced when 9.81 gg of butane reacts with excess oxygen. Express your answer to three significant figures and include the appropriate units.
Butane, C4H10C4H10, reacts with oxygen, O2O2, to form water, H2OH2O, and carbon dioxide, CO2CO2, as shown in the following chemical equation: 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) The coefficients in this equation represent mole ratios. Notice that the coefficient for water (10) is five times that of butane (2). Thus, the number of moles of water produced is five times the number of moles of butane that react. Also, notice that the coefficient for butane (2) is one-fourth the coefficient of carbon dioxide (8). Thus, the number of moles of butane that react is one-fourth the number of moles of carbon dioxide that you produce. But be careful! If you are given the mass of a compound, you must first convert to moles before applying these ratios. A) Calculate the mass of water produced when 7.34 g of butane reacts with excess oxygen. Express your answer to three digits. B) Calculate the mass of butane needed to produce 94.6 g of carbon dioxide.

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