50.00g of compound A (molar mass=56.48g/mol) and 17.56g compound B (molar mass = 49.60 g/mol) react completely to form 9.91g compound C (molar mass = 27.93 g/mol) and 57.65g compound D (molar mass = 81.43 g/mol) with neither reactant in excess. what is the coefficient for compound A in the chemical equation for this reaction when balanced in lowers whole-numbers?

50.00g of compound A (molar mass=56.48g/mol) and 17.56g compound B (molar mass = 49.60 g/mol) react completely to form 9.91g compound C (molar mass = 27.93 g/mol) and 57.65g compound D (molar mass = 81.43 g/mol) with neither reactant in excess. what is the coefficient for compound A in the chemical equation for this reaction when balanced in lowers whole-numbers?

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 50A

See similar textbooks

Similar questions

combustion of a compound of formula CxHyOz yields 0.209g H2O (molar mass = 18.016 g/mol) and 0.512g CO2 (molar mass=44.01g/mol) when 0.497g of O2 (molar mass =32g/mol) is used. Based on this combustion analysis data, what mass of oxygen is from the mass of compound combusted and not from the oxygen gas used to combust the compound?
If you start with a mixture of Nacl and KClO3 that weighs 3.00g, and the mass of the sample decreased by 0.75g after heating, what is the best explanation for the change in mass? -0.75g KClO3 and NaCl reacted to form products -0.75g O2 was formed in the reaction and left the same sample as gas -0.75g KCl was formed -0.75g KClO3 reacted to form products or.. -0.75g NaCl reacted to form products
What mass of carbon dioxide (molar mass 44 g /mol) is produced by the burning of 2 gallons (5340g) of gasoline? (Consider gasoline as C8 H18) (Hint: molar ratios, and need to convert.)
Propenoic acid, C3H4O2, is a reactive organic liquid thatis used in the manufacturing of plastics, coatings, and adhesives.An unlabeled container is thought to contain thisliquid. A 0.275-g sample of the liquid is combusted to produce0.102 g of water and 0.374 g carbon dioxide. Is the unknownliquid propenoic acid? Support your reasoning withcalculations.
Glucose (C6H12O6) can be fermented to yield ethanol (CH3CH2OH) and carbon dioxide (CO2). C6H12O6⟶2CH3 CH2 OH+2 CO2 The molar mass of glucose is 180.15 g/mol,, the molar mass of ethanol is 46.08 g/mol, and the molar mass of carbon dioxide is 44.01 g/mol. What is the theoretical yield of ethanol from the fermentation of 69.0 g of glucose? If the reaction produced 23.4 g of ethanol, what is the percent yield?
A mixture of BaO and CaO weighing 2.2120g is transformed into mixed sulfates, BaSO4 and CaSO4 weighing 5.0230g. Calculate the number of grams CaO and BaO in the mixture. What weight of limestone should be taken so that 1/20 the number of mg of CaSO4 obtained will represent the percentage of CaO in the numeral?
Aspirin, acetylsalicylic acid (C9H8O4), is produced by the reaction of salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) according to the following: C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2. In a certain aspirin synthesis, 104.8 g of salicylic acid and 110.9 g of acetic anhydride are combined. Calculate the percent yield of the reaction if 105.6 g of aspirin are produced.
Glucose can be fermented to yield ethanol and carbon dioxide. a. What is the theoretical yield of ethanol (in grams) produced with a 66% yield and an actual yield of 29.6g? b. What is the mass of the glucose (in grams) in the fermentation reaction?
An alloy is found to be 41.8% Zn and the rest is Cu. If 15.0 g of Cu is added to 45.0 g of This alloy , what will be the new percentage of Cu in the alloy ?
Aspirin, C₉H₆O₄, is prepared by reacting salicylic acid, C₇H₆O₃, with acetic anhydride, C₄H₆O₃, in the reaction:2C₇H₆O₃ + C₄H₆O₃ → 2C₉H₆O₄ + H₂OA student is told to prepare 22.0 g of aspirin. He is also told that he should use a 50.0% excess of acetic anhydride and expect to get a 64.0% yield in the reaction.How many grams of salicylic acid, C₇H₆O₃, should he use? And how many grams of acetic anhydride, C₄H₆O₃, should he use?
A student starts with 0.627 g0.627 g of pure 4‑aminobenzoic acid, (molar mass 137.14 g/mol137.14 g/mol) and ends up with 0.619 g0.619 g of benzocaine (molar mass 165.19 g/mol165.19 g/mol). Given that ethanol is in excess, what are the theoretical and percent yields for this reaction? Assume all starting material is converted to product when calculating the theoretical yield.
3.50g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 176./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 5.25g water 1.43g Use this information to find the molecular formula of X