INFORMATION ABOUT CHEMICAL REACTIONStudy→ Previous Page 5 of 11Black smokers are found in the depths of the oceans. Thinking that theconditions in these smokers might be conducive to the formation of organiccompounds, two chemists in Germany found the following reaction could occurin similar conditions.2 CH3 SH + CO → CH3COSCH3 + H₂SIf you begin with 47.2 g ofCH3 SH and excessCO, what is the theoretical yield ofCH3COSCH3?Next →g CH3 COSCH3Save and ExitIfyou isolate 22.6 g ofCH3COSCH3, what is the percent yield ofCH3COSCH, ?%Submit Q

theoretical yield and percentage yield

pounds, two chemists in Germany found the following reaction could occ in similar conditions. 2 CH3 SH + CO → CH3COSCH3 + H₂S If you begin with 47.2 g of CH3 SH and excess CO, what is the theoretical yield of CH3COSCH3? g CH3 COSCH3 If you isolate 22.6 g of CH3COSCH3, what is the percent yield of CH3COSCH, %

pounds, two chemists in Germany found the following reaction could occ in similar conditions. 2 CH3 SH + CO → CH3COSCH3 + H₂S If you begin with 47.2 g of CH3 SH and excess CO, what is the theoretical yield of CH3COSCH3? g CH3 COSCH3 If you isolate 22.6 g of CH3COSCH3, what is the percent yield of CH3COSCH, %

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 a certain ecperiment, 50 g of sodium chloride is reacted with 75.0 g of sulfuric acid, and 52.0g of sodium sulfate is produced. Determine the percent yield for this reaction. Unbalanced equation: NaCl (s) +H2SO4(i) -> HCl(g) + Na2SO4(s)
If the theoretical yield of H20 in the reaction is 49.3 grams, and 16 grams are actually produced, what is the % yield of H2O? 2 H2 + O2 --> 2 H2O Round your answer to 2 decimal places.
fill in the way it asks please and calculate % yeild.
In this reaction: Mg (s) + I₂ (s) → MgI₂ (s), if 10.0 g of Mg reacts with 60.0 g of I₂, and 61.96 g of MgI₂ form, what is the percent yield?
A) Determine the molecular formula of X (the starting reagent) B) Write a balanced equation for this reaction C) Determine the theoretical mass of the CO2 produced if 0.2 mol of O2 is completely consumed D) If the combustion reaction produced is 3.0g of CO2, determine its percentage yield
Combining 0.376 mol Fe₂O3 with excess carbon produced 20.0 g Fe. Fe₂O3 + 3C2Fe + 3 CO What is the actual yield of iron in moles? actual yield: What is the theoretical yield of iron in moles? theoretical yield: What is the percent yield? percent yield: mol mol %
In this reaction: Mg (s) + I₂ (s) → MgI₂ (s) If 2.38 moles of Mg react with 3.56 moles of I₂, and 1.76 moles of MgI₂ form, what is the percent yield?
In this reaction: Mg (s) + I₂ (s) → MgI₂ (s) If 2.58 moles of Mg react with 3.56 moles of I₂, and 1.76 moles of MgI₂ form, what is the percent yield?
How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic
In this reaction: Mg (s) + I₂ (s) → MgI₂ (s), if 10.0 g of Mg reacts with 60.0 g of I₂, and 63.40 g of MgI₂ form, what is the percent yield?
For the reaction SO3 + H2O→ H2SO4, calculate the % yield, if 343 grams of SO3 react with excess water to produce 104g H2SO4
Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 1.44g of carbon dioxide is produced from the reaction of 0.60g of ethane and 3.7g of oxygen gas, calculate the percent yield of carbon dioxide.