Medicare does not cover the cost of this prescription medicine, which currently averages $297.78 per kilogram.   The theoretical yield for the pure barium sulfate you were transferring was 500.00kg.   You spilled 27.45 kg.   What is the % yield of the transfer that you need to report?  And also determine the consumer price of the spilled barium sulfate.

Balance the following chemical equation and determine the number of moles of Fe(s) produced when 1 moles of Fe203(s) react with excess C(s) to produce Fe(s) and CO2(g). Fe203(s) + C(s) → Fe(s) + CO2(g) O Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105)

Use 1 decimal point for all atomic masses. 12.3 g of NCl3(g) are reacted with 0.605 g of H2(g) by the following reaction   NCl3(g) + 3H2(g) --> NH3(g) + 3HCl(g) What is the limiting reagent? NCl3(g) H2(g)     Based on the limiting reagent, what should the yield of NH3(g) be?

For the following reaction, 3.75 grams of sodium are mixed with excess water. The reaction ylelds 4.91 grams of sodium hydroxide. sodium (s) + water (I) sodium hydroxide (aq) + hydrogen (g) What is the theoretical yield of sodium hydroxide ?| What is the percent yleld of sodium hydroxide ? grams

How do I answer this question while also following the format?

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

Yeast converts glucose (C6H1206) into ethanol (d = 0.789 g/mL) in a process called fermentation. An unbalanced equation for the reaction can be written as follows: CH₁206(aq) C₂H₂OH(1) + CO₂(g) - Balance this fermentation reaction by adding the missing coefficients. X X₁ He d. 1 C6H₁2O6(aq) - 2_C₂H₂OH(1)+ 2_CO₂(g) If 350.0 g of glucose yields 142.0 mL of ethanol, what is the percent yield for the reaction? % See Periodic Table See Hint

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

[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.

Zinc sulfide reacts with oxygen according to the reaction2ZnS(s) + 3O2 (g)› 2ZnO(s) + 2SO2 (g)A reaction mixture initially contains 4.8 mol ZnS and 8.9mol O2Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains? Express your answer using two significant figures.