No Lr |252) (257) (258) (259) (262) and Physical Sciences 2017 2. For the following balanced equation, indicate how many moles and grams of each reactant and product are needed/produced in the reaction. Show your work (mole-ratio etc...), fill in the blanks. 3 B2H6 + 6 NH3 2 B3H6N3 + 12 H2 22.2 g C17mol mol mol mol 22.29 Imol B2 HG (2x10,81)+6x1.0oB2Ha 14,0t(3x1.00f)NH> IMOINH, 3molBa Hc ス1.6ス 6.0up 27.67

No Lr |252) (257) (258) (259) (262) and Physical Sciences 2017 2. For the following balanced equation, indicate how many moles and grams of each reactant and product are needed/produced in the reaction. Show your work (mole-ratio etc...), fill in the blanks. 3 B2H6 + 6 NH3 2 B3H6N3 + 12 H2 22.2 g C17mol mol mol mol 22.29 Imol B2 HG (2x10,81)+6x1.0oB2Ha 14,0t(3x1.00f)NH> IMOINH, 3molBa Hc ス1.6ス 6.0up 27.67

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 hydrated salt, MY3·xH2O, was heated strongly in a crucible to remove all the watermolecules of crystallization.The data are for this experiment are given in the table below.Mass of empty crucible and cover 29.73 gMass of crucible, cover, and hydrated salt 32.72 gMass of crucible, cover, and anhydrous salt 31.52 gMolar mass of anhydrous salt 241.88 g/mol(i) Calculate the % composition by mass of water in the hydrated salt.(ii) Determine the value of x.(iii) M is in Period 4 of the Periodic Table of the Elements.If Y = NO3–, identify the element M.(iv) What is the name of this hydrated salt? ___
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In batteries factory, the manager asked the technician to prepare a batch of battery acid with a concentration of 23.6% (wt %) as follows Raw materials (streams) Stream 1: Old weak battery acid (H2SO4) solution contains 16.9% (wt %) of H2SO4 (the rest is pure water) Stream 2:250 kg of 65.2 % H2SO4 How many kilograms of old weak battery acid (H2SO4) are needed to prepare the desired ?battery acid (23.6%) .a o 3313.43 Kg bo 1755.25 Kg .CO 1552.24 Kg .do 3875.14 Kg
Q2: A fuel oil is burned with 65% excess air, and the combustion characteristics of thefuel oil are similar to a paraffin series dodecane C12H26. Determine: (a) the actualair/fuel ratio (A/F) on a mole basis, (b) the actual air/fuel ratio (A/F) on a mass basis,and (c) the actual volumetric (molar) analysis of the products of combustion. State allthe assumptions that you would made before solving this question. Air contains 21%O2 and 79% N2 by mole. Do not solve in tabulated form.
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Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L
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C9H8O4 is synthesized by reacting stoichiometric amounts of C7H6O3 and (CH3CO)2O, as shown by the balanced chemical equation in the picture: During the synthesis, 500 grams of salicylic acid was available for use in the experiment. Other information: MW of Salicylic Acid: 138.121 g/mol MW of Acetic Anhydride: 102.09 g/mol Density of Acetic Anhydride: 1/08 g/ml Question: The available Acetic anhydride reagent in the lab is in the liquid form. How many mL of Acetic anhydride is needed to react with the available salicylic acid stoichiometirically?
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurFormulation: 250 mg per jarDosage form: Ointment Packaging: 100 jars per boxWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2SMy problem: Find the number of dosage form and packaging that can be produced from the stoichiometric calculation based on the result upon finding the Mass to Mass Stoichiometry Calculation. I have based my answer to the mass stoichiometry from this link: https://www.bartleby.com/questions-and-answers/given-raw-materials-500-g-calcium-polysulphide-and-1.5-kg-hydrochloric-acid-actual-yield-343.4g-prec/b1de1102-f27f-4c8d-9b4e-c7fe8e6104b6Thanks, by the way. But can you still help me find the number of dosage from and packaging?
A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)