Can someone provide a step-by-step answer for the following blanks in the second table? Thank you in advance! :) ActiveRaw Materials Actual Yield Formulation Dosage FormPackagingIngredient500 g calciumpolysulphideand 1.5 kg343.4gprecipitated250 mg perjarPrecipitated100 jars perboxOintmentsulfurhydrochloricsulfuracidIC. SYNTHESIS AND PACKAGingBalanced Chemical Reaction% composition by mass of each compoundMass to Mass Stoichiometry CalculationLimiting ReagentExcess ReagentAmount (g) in excess% YieldNumber of dosage form and packaging that canbe produced from stoichiometric calculation

Active Raw Materials Actual Yield Formulation Dosage Form Packaging Ingredient 500 g calcium polysulphide and 1.5 kg hydrochloric 343.4g precipitated sulfur Precipitated sulfur 250 mg per jar 100 jars per box Ointment acid IC. SYNTHESIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation

Active Raw Materials Actual Yield Formulation Dosage Form Packaging Ingredient 500 g calcium polysulphide and 1.5 kg hydrochloric 343.4g precipitated sulfur Precipitated sulfur 250 mg per jar 100 jars per box Ointment acid IC. SYNTHESIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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Given: Active Ingredient: Potassium Nitrate Raw Materials: 3 kgs. acetic acid and 2.5 kgs. potassium bicarbonate Actual Yield: 1.66 kgs. potassium acetate Formulation: 1100 mg per 5 mL Dosage Form: Oral Solution Packaging 473 mL per bottle Synthesis and Packaging (Need answer)Balanced Chemical Equation: % composition by mass of each compound: Mass to Mass Stoichiometry Calculation: Limiting Reagent: Excess Reagent: Amount (g) in excess: % Yield: Number of dosage form and packaging that can be produced from stoichiometric solution:
Balance, what is he coefficient in front H2SO4?
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?
Calculate the ratio between the moles of magnesium used and the moles of oxygen used. Express this ratio in simplest whole-number form. Mass of oxygen = 0.49g- 0.33g= 0.16gNumber of moles = given mass / molar massNumber of moles of oxygen = 0.16/ 16 = 0.01 molMolarmass of magnesium = 24.3gMoles of magnesium = 0.33g / 24.3g = 0.0135 molMoles of magnesium 0.0135 1.35 3 4------------------------ = _____________ = ____________ x ________ = ___Moles of oxygen 0.01 1 3 3 The ratio between the moles of magnesium used and the moles of oxygen uses is 4/3. Based on your experimental data, write the empirical formula for magnesium oxide. Is this the molecular formula or the simplest formula? Explain how you know this.
The combustion of liquid ethanol (C2H5OH)(C2H5OH) produces carbon dioxide and water. After 4.63 mLmL of ethanol (density=0.789g/ml)(density=0.789g/ml) was allowed to burn in the presence of 15.50 gg of oxygen gas, 3.70 mLmL of water (density=1.00g/ml)(density=1.00g/ml) was collected. Determine the theoretical and percent yeild of h2o in the reaction.
You own a pharmaceutical company that is manufacturing the experimental drug inhaler for COVID-19 disease and produce lower production yield as compared to a leading pharmaceutical company. Explain why production yield is low, using the concepts on a. limiting and excess substance, b. law of supply and demand.
Using the data collected (e.g., masses of hydrated metal salt and oxalic acid 1M reacted and actual yield of hydrated metal oxalate precipitate) and the balanced reaction for the formation of the metal oxalate product determine: 4.031g of ammonium iron (II) sulfate hexahydrate concentration of oxalic acid : 50mL of 1M oxalic acid ferrous oxalate dihydrate was formed weighed (Actual Yield) 1.746g. 1. identity of the limiting reactant in the synthesis of ferrous oxalate, 2.Theoretical yield of the ferrous oxalate dihydrate complex, and 3.The per cent yield of the ferrous oxalate dihydrate product of this reaction.
underecfectsol
The reaction of solid calcium fluoride and sulfuric acid produces calcium sulfate solids and gaseous HF. The gas product is dissolved in water to form hydrofluoric acid. Fluorite ore, a source of calcium fluoride, contains 95%wt CaF2 and 5%wt SiO2. In a certain process, the ore is reacted with 93%wt aqueous sulfuric acid, supplied 15% in excess. From this, 95% of the ore dissolves in the acid. Some of the HF formed reacts with the dissolved silica in the reaction: HF reacts with SiO2 to produce H2SiF6 and liquid water. If 60%wt of hydrofluoric acid was formed when hydrogen fluoride (which exits the reactor) is dissolved in water, determine the amount of ore needed to produce one metric ton of acid. Report your answers to one decimal place only.
Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is C12H22O11 + H2O + 3O2 --> 2C6H8O7 + 4H2O Using a metric ton(1000kg) of sucrose the expected yield is 1122Kg. On average if only 1036kg is produced, what is the % yield for this reaction?
You are supplied with 1150 kg ethanol (C2H5OH), together with methanol (CH3OH), potassium hydroxide (KOH) and ammonia (NH3). You are requested by a customer to produce methyl acetate (CH3COOCH3), potassium acetate (CH3COOK) and ammonium acetate (CH3COONH4) in mass forms. (a) Calculate the mole & mass of acetic acid (CH3COOH) converted from ethanol through excessive oxidation.
Use your balanced chemical reaction from the above problem. How many kilograms of the barium product can be produced at 100% yield from the double replacement reaction, made in industry at a larger scale of 675.00 pounds of barium nitrate that is then dissolved in water and mixed with an excess of the potassium sulfate solution. The product is collected by gravimetric filtration and dried. Use 453.592 g = 1 lb. Ba(NO3)2 + K2SO4 ---> BaSO4 + 2KNO3