30) What is the percent yield for the reaction below? Only 28.16 g of CO2 are observed to have formed even though stoichiometry would predict the production of 225.3 g of CO2 since 4.000 (l00 moles of C8H18 and 8.000 moles of O2 were used. 2 C3H18 + 25 O2 16 CO2 + 18 H2O A) 12.50% B) 25.00% C) 50.00% 20.00%

30) What is the percent yield for the reaction below? Only 28.16 g of CO2 are observed to have formed even though stoichiometry would predict the production of 225.3 g of CO2 since 4.000 (l00 moles of C8H18 and 8.000 moles of O2 were used. 2 C3H18 + 25 O2 16 CO2 + 18 H2O A) 12.50% B) 25.00% C) 50.00% 20.00%

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section3.8: Evaluating Chemical Synthesis: Percent Yield

Problem 3.18PSP: Assume the methanol synthesis has an 85.0% yield and you want to make 1.00 kg CH3OH. Calculate the...

See similar textbooks

Similar questions

Give the theoretical yield, in moles, of CO2 from the reaction of 0.60 moles of C8H18 with 40.00 moles of O2. 2C8H18+25O2 ---> 16CO2 + 18H2O
Suppose 7.0g of Compound A and 3.5g of Compound B are consumed in a reaction that produces only one product, Compound C . Calculate the theoretical yield of C . Round your answer to the nearest 0.1g . 10.5g Suppose 6.5g of C are actually isolated at the end of the reaction.What is the percent yield of Compound C ? Round your answer to the nearest whole percent. %
Phthalonitrile (C₈H₄N₂) is produced by the ammoxidation of o-xylene (C₈H₁₀) according to the following reaction: C₈H₁₀(l) + O₂(g) + NH₃(g) → C₈H₄N₂(s) + H₂O(l) How many grams of water would be produced by the complete ammoxidation of 17.8 moles of o-xylene?
Calculate the percent yield for an experiment in which 8.50g of SOCl2 was obtained in a reaction of 6.80g of SO2 with excess PCl5. Use the following equation: SO2 (l) + PCl5 (l) → SOCl2 + POCl3
Phthalonitrile (C₈H₄N₂) is produced by the ammoxidation of o-xylene (C₈H₁₀) according to the following reaction: C₈H₁₀(l) + O₂(g) + NH₃(g) → C₈H₄N₂(s) + H₂O(l) How many moles of water would be produced by the complete ammoxidation of 137.5 grams of o-xylene?
A)What mass of ammonia gas can be produced from a reaction between 565.0g H2 and 880.0g of N2 through the Harber-Bosch reaction? B)What mass of the excess reagent remains? N2(g)+3H2(g)-->2NH3
Calculate the precent yield if 10.0 g of P4O10 is isolated from the reaction shown below if 6.0 grams of P4 was used and O2 is used in extreme excess. P4 + 5O2---> P4O10
The 2-step process for melamine is: CO(NH2)2(l)→HNCO(l)+NH3(g) 6HNCO(l)→C3N3(NH2)3(l)+3CO2(g) What mass of melamine, C3N3(NH2)3, will be obtained from 189.0 kg of urea, CO(NH2)2, if the yield of the overall reaction is 70.0 % ?
Calculate the percent yield if 4.4g of P4 reacts with 20g of O2 to yield 4.3g of P4O10 from the reaction. P4 + 5O2 -> P4O10
3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.54 kgkg of H2H2 and 34.1 kgkg of N2N2?
Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2C8H18+25O2 ---> 16CO2 + 18H2O A. 2.56 mol B. 0.646 mol C. 6.4 mol D. 16 mol
Given the following balanced reaction, Fe2O3+3C-->2Fe+3CO if 1140 of fe2o3 were reacted with ecess c, what would be the percent yield for the reaction if 455g of CO were actually collected? density fe2o3=5.24g/cm3, density of co is 1.14kg/m3