Use this table to answer the following questions below: Before reaction Before reaction Theoretical yield Theoretical yield Actual yield Yes, it is balanced. Other: Is the chemical reaction involved balanced? If not, kindly type the correct balanced equation. Please take note that subscripts cannot be written properly. What is the percentage yield in this experiment? * 96.3% 93.6% CH3OH 32.0 g 1.00 mol 36.9% O 63.9% CO Excess Excess CH3COOH 0 0 1.00 mol 60.0 g 57.8 g

Use this table to answer the following questions below: Before reaction Before reaction Theoretical yield Theoretical yield Actual yield Yes, it is balanced. Other: Is the chemical reaction involved balanced? If not, kindly type the correct balanced equation. Please take note that subscripts cannot be written properly. What is the percentage yield in this experiment? * 96.3% 93.6% CH3OH 32.0 g 1.00 mol 36.9% O 63.9% CO Excess Excess CH3COOH 0 0 1.00 mol 60.0 g 57.8 g

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...

See similar textbooks

Similar questions

In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 120 g 240 g 38.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) 2.5 g Al, 2.5 g Cl2 Express your answer using two significant figures. 7.4 g Al, 24.4 g Cl2 Express your answer using three significant figures. 0.230 g Al, 1.20 g Cl2 Express your answer using three significant figures.
Combining 0.288 mol Fe,0, with excess carbon produced 16.2 g Fe. Fe,0, +3C – 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: mol What is the theoretical yield of iron in moles? theoretical yield: mol What is the percent yield?
1.0 chem q
TABLE 3. PERCENT YIELD Mass salicylic acid 9 Mass of synthesized aspirin g 9 Theoretical Yield (aspirin) Percent Yield % Calculations: Note: Show calculations in a separate bond paper. (For the percent yield, you must first determine the limiting reactant from the following data: molar mass of salicylic acid = 138 g; molar mass of acetic anhydride = 102 g; density of acetic anhydride = 1.08 g/mL). TABLE 4. MELTING POINT DATA Sample Melting Point Range salicylic acid synthesized aspirin
Combining 0.333 mol Fe, O, with excess carbon produced 12.7 g Fe. Fe,0, + 3C → 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: mol What is the theoretical yield of iron in moles? theoretical yield: mol What is the percent yield? percent yield: %
Question 25 of 97 Submit DDT was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. It can be prepared by the reaction shown below. Determine the amount of DDT that can be produced and the percent yield for this reaction. 2C6H,CI + C2HOCI, – C,4H9CI, + H20 2 3 NEXT If a company in South America started with 1175 g of chlorobenzene (C6H5CI, MW 112.55 g/mol) and 538.5 g of chloral (C2HOCI3, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2C6H,CI C2HOCI, C1.H,Cls H2O Before (mol) Change (mol) After (mol) O RESET 3.132 -3.132 3.654 -3.654 7.308 0. + -7.308 10.44 -10.44 MacBook Air F12 II F8 F10 F11 000 F9 20 F3 F7 F4 F5 F6 esc F2 F1 +.
Consider the reaction between sodium sulfide and copper(Il) sulfide: NazS (aq) + CuS04 (aq) -> Na2SO4(aq) + CuS (s) A chemist allows 16.7 g of Na,S and 35.0 g of CUSO, to react. Determine the theoretical yield of NazSO4 for the reaction. 31.1 20.5 30.4 O 21.0
Please don't provide handwritten solution
8 This is for my reviewer please help me with the step by step solution and answer, thank you
How many grams of NaCl should be produced if you start with 1.0 g of sodium bicarbonate. This conversion will require three conversion factors. Start with 1.0 g NaHCO3. Then use a conversion factor that converts that to moles. Then use the balanced equation to convert from moles of NaHCO3 to moles of NaCl. Then use a conversion factor to convert to grams.
What is the relationship between limiting reactant and theoretical yield? The limiting reactant is the reactant that runs out, so it will determine the theoretical yield of product The limiting reactant is the reactant that is put in first, so it will determine the theoretical yield of product The limiting reactant is the reactant you have the most of, so it determines the theoretical yield of product The limiting reactant is the reactant you have less of, so it determines the theoretical yield of product