lr___yield_lab

B. Stoichiometry and Percent Yield DATA 1. Mass of sodium carbonate 2. Mass of filter paper 3. Mass of dry filter paper and calcium carbonate product CALCULATIONS AND QUESTIONS (show all of your work) 1. Mass of dried product (actual yield) (Mass of dry filter paper and calcium carbonate product - mass of filter paper) 1.0 g 1.2g 2.69 2. Write the balanced chemical equation for the reaction of sodium carbonate and calcium chloride. (Ignore the hydrate in this equation) 2.89 3. Use stoichiometry to calculate the theoretical yield of calcium carbonate product based on the starting mass of sodium carbonate. 4. Calculate the percent yield of the reaction based on the actual yield of dried calcium carbonate product and the theoretical yield of calcium carbonate product. 11

5.In a lab setting, a student obtained 9.60 g of AgCl from the reaction listed below. The student added 14.1 g Hydrochloric acid to 14.1 g of Silver sulfate. 2HCl + Ag2SO4 --> 2AgCl + H2SO4 What is the percent yield of the AgCl obtained from the lab experiment? ______ % yield All work must be shown and submitted. Any steps left out may result in a loss of points for that particular problem.   ALL UNITS AND LABELS MUST BE SHOWN THROUGHOUT THE PROBLEM, INCLUDING CANCELLING THEM WHEN APPROPRIATE. If units and/or labels are missing, 2 points will be deducted per problem.

I make a product and weigh it before it is dry. Does that affect the actual yield? Yes No Check it GET A HINT * SCRATCHPAD * Improve this question

Percent Yield

Percent yield

Mass of vial + AgNO3 __16.9209g Mass of empty Vial ________6.8951g   Mass of copper wire BEFORE the reaction ____4.3168g Mass of copper wire AFTER the reaction _____2.6851g   Mass of filter paper __0.7253g Mass of filter paper with dry silver ______6.3254g   Calculations: Please do the following three calculations, showing the math set-up for each.  Mass of AgNO3 used in reaction (this is the mass of just the AgNO3, without the vial) Mass of copper wire consumed in the reaction (this is the mass of the Cu that was used up in the reaction, NOT the mass of the entire wire) Mass of silver metal produced in reaction (this is your EXPERIMENTAL yield, NOT including the mass of the filter paper)!

How many grams of N2 are needed to completely (stoichiometrically) react with  222 g of Br2 ?  N2   +   3 Br2   →   2 NBr3   +   44.0 kJ              The molar mass of Br2 is _____________ g and the molar mass of N2 is  ___________ g                                ____________ mol Br2                                                              (2.22 x 102 g Br2)(––––––––––––––––––––––––––––––)  =  __________ mol Br2                               _______________ g Br2                                                                                                                       ______________ mol N2 __________________ mol Br2 (–––––––––––––––––––––––––) =  _______________ mol N2                                                     __________________ mol Br2                                                       ___________________ g N2 _______________ mol N2 (–––––––––––––––––––––––––) =  _____________ g N2                                                    ________________ mol N2

please answer the theortical yield

Multiple Choice. Read and analyze each question. Write the letter that corresponds to your answer on a separate sheet of paper. 1. Suppose your classmates will be visiting you. You decided to make burger for their snack. You have 20 burger patties and 17 burger buns, how many burgers you can make? а. 20 b. 17 с. 3 d. 37 2. Based on problem 1, what is the limiting reactant? a. burger buns b. burger patties c. your classmates d. your budget 3. Based on problem 1, how many burger patties are extra after your preparation for snack? с. 17 d. 3 a. 0 b. 37 For numbers 4-10. If 68 g of Zn reacts with 27.5 g of HC1. Use the chemical equation to answer the following questions below. Zn + 2HC1 ZnCl2 + H2 4. What is the molar mass of Zn? a. 65 g/mol b. 30 g/mol c. 27 g/ mol d. 68 g/ mol 5. What is the molar mass of HC1? a. 2 g/mol b. 16 g/mol 6. What coefficient is indicated in HCl? c. 36 g/mol d. 68 g/mol c. 4 d. 5 a. 2 b. 3 7. Which substance is limiting reactant? a. ZnCl2 b. HCl 8. Which…

The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:4 NH3(g) + 7 O2(g) à 4 NO2(g) + 6 H2O(g)The combustion of 28.8 g of ammonia consumes __________ g of oxygen. please explain the step by step procedure

what is the total mass in grams for the collection of all three elements? 

Calculate the theoretical mass and the percent yield. Please show all work!

I. Procedure, Results and Observations: 1. Butane is typically used as fuel for cigarette lighters and portable stoves. A. What substance is required for the complete burning of butane? B. Balanced chemical equation for the combustion of butane: C. Calculation: If 74.3 g of butane is burned in 132 kg of oxygen a. Which is the limiting reagent? b. What is the mass of carbon dioxide obtained by heating butane? c. How much of the excess reagent remains unreacted?

Stoichiometry WS #1 (DA Review) 1. How many seconds are there in 2.5 years? 2. An average human heart beats 60. times per minute. If you live to be 82 years old, how many times will your heart beat?

For this reaction: How many moles of carbon dioxide will be produced when 6.00 mols of oxygen reacts with 1.25 moles of C3H7SH? help!   C3H7SH + 6 O2 ---><--- 3 CO2 +SO2 + 4 H2O a. 1.25 moles b. 2.50 moles c. 3.00 moles d. 4.00 moles e. 6.00 moles

Is the number of total molecules on the left side of a balanced equation always equal to the number or total molecules on the right side of the equation?

Table 1 1. Volume of vinegar (mL) 2. Volume of water (mL) 3. Mass of beaker with liquid (g) 4. Mass of Alka Seltzer tablet (g) 5. Total Starting Mass (g) = 3. + 4. 6. Mass of beaker with liquid after bubbles cease (g) 7. Calculated mass of CO2 lost (produced) (g) <= 5.-6. This is g CO2 8. Calculated mass of NaHCO3 reacted (g) Use Stoichiometry: g CO2 →g NaHCO3 Run 1 0.00 Run 2 0.7 5ML 10ml 30ml 136.427 146.243 30ml Run 3 Run 4 15ml 0.772 0.926 Run 5 20ml 0.929 Run 6 25ml 25ml 20ml 146.459 146.52g| 144.387 146.947 іни. Run 7 15ml 10ml 5ml Run 8 30ml 35m1 0.00 8.243g 3.2439 3.235 6.259 3.239 3.24 g 3.23g 139.87 149.486 149.48 149.75 149.617 150.207 149.884 139.179 148.7149 148.7549 148.821g|148.700g|148.270g| 148.931g|149.431g 0.917 1.937 -0.047 0.9 146.454 147.3110 3.23g 3.22g 150.53

How many moles of W are needed to react with 1.0 mol of Ho in the hypothetic chemical reaction? 3W + 2Ho  →  2W3Ho   a. 0   b. 1.5   c. 2   d. 3   e. 1

If you forget to weigh the calorimeter and contents at the end of a Part 1 run, you will: Select one: a. Use the mass from another run to do the calculations. b. Guess what the final mass should be. C. Put about the same volume of solutions in the calorimeter and weigh it. d. Do another run.

Dosage Form Active Raw Materials Actual Yield Formulation Packaging Ingredient 3 kgs. p-aminophenol and 2 kgs. acetic anhydride 20 tablets 2.6 kgs paracetamol 500 mg per per blister рack Paracetamol Tablet tablet 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

Use the References to access important values if needed for this question. Consider the following unbalanced particulate representation of a chemical equation: I= purple F= green Write a balanced chemical equation for this reaction, using the smallest integer coefficients possible. Do not include states. Submit Answer Retry Entire Group 7 more group attempts remaining +తల + +

Balance the reaction shown below:   H2CO3+NaOH→Na2CO3+H2OH2CO3+NaOH→Na2CO3+H2O  Once balanced, given 0.367 moles H2CO3H2CO3, calculate the grams of H2OH2O produced. A. 1.65 B. 38.3 C. 13.2 D. 61.8 E. 16.9

The actual yield can only be determined by: 8°F Mostly cloudy O Writing a balanced equation. O Calculating the theoretical yield and plugging into the percent yield. O Reviewing past reactions. O Carrying out the reaction in a laboratory. O Search H

Please answer the question "Number of dosage form and packaging that can be produced from stoichiometric calculation."

Balance the reaction first. Show all work. Report answers in proper significant figures.

two partners were trying to solve the equation. Penny Said that the equation is balanced because there is only 1 Fe on both sides of the equation. But Alex disagrees. Who is correct and why? Write the CER to explain your answer. claim: Evidence: Reasoning

Show all calculations and steps: 10. Determine the amount (in moles) of 2.35 kg of hydrogen sulfate. Show all work.