Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 55.%. Suppose 4.0 g of A are reacted with excess Compound B, and 5.5 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much B was consumed by the reaction? ? Round your answer to the nearest 0.1 g. olo

Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 55.%. Suppose 4.0 g of A are reacted with excess Compound B, and 5.5 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much B was consumed by the reaction? ? Round your answer to the nearest 0.1 g. olo

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.44PAE: 4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of...

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When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
The combustion of liquid chloroethylene, C2H3Cl, yields carbon dioxide, steam, and hydrogen chloride gas. (a) Write a balanced equation for the reaction. (b) How many moles of oxygen are required to react with 35.00 g of chloroethylene? (c) If 25.00 g of chloroethylene react with an excess of oxygen, how many grams of each product are formed?
4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
When benzene (C6H6) reacts with bromine (Br)2, bromobenzene(C6H5Br) is obtained:C6H6 + Br2-------->C6H5Br + HBr(a) When 30.0 g of benzene reacts with 65.0 g of bromine, whatis the theoretical yield of bromobenzene? (b) If the actual yieldof bromobenzene is 42.3 g, what is the percentage yield?
Apidic acid (H2C6H8O4) is used to produce nylon. Apidic acid is made commercially by a reaction between cyclohexane (C6H12) and oxygen (O2). What is the balanced reaction for this transformation? (Hint: Water is formed as a by-product.) Assume that cyclohexane is the limiting reagent. You start with 25.0 g of cyclohexane. How much apidic acid could be produced? c. In reality, you only made 33.5 g of apidic acid. What is your % yield for the reaction?
When 12.10g of MTBE (methyl tert-butul ether) is burned in a combustion apparatus with oxygen, it forms 30.20g of CO2 and 14.80g of H20. Given the compound molar mass (88.17)g/mol - what is the Molecular Formula of the compound ?
Diethyl ether (C4H10O)(C4H10O), the "ether" used medically as an anesthetic, is prepared commercially by treatment of ethyl alcohol (C2H6O)(C2H6O) with an acid. How many grams of diethyl ether would you obtain from 58.8 gg of ethyl alcohol if the percent yield of the reaction is 90.0 %% ? 2C2H6O(l)Ethyl alcohol−→−AcidC4H10O(l)Diethyl ether+H2O(l) Round to 3 sigfigs in answer (they didn't accept 41.6 grams as the answer)
Suppose 1.0g of Compound A and 9.5g 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. Suppose 9.6g 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.
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Yeast converts glucose (C6H12O6) into ethanol (d=789g/mL) in a process called fermentation. An equation for the reaction can be written as follows: If 100.0g of glucose yields 50.0mL of ethanol, what is the percent yield for the reaction?
Aniline (C6H5NH2) can be produced from chlorobenzene (C6H5Cl) via the following reaction: C6H5Cl (l) + 2 NH3 (g) ⟶ C6H5NH2 (l) + NH4Cl (s) Assume that 20.0 g of chlorobenzene at 92% purity is mixed with 8.30 g of ammonia. a) Which is the limiting reactant? b) Which reactant is present in excess? c) What is the theoretical yield of ammonium chloride in grams? d) If 4.78 g of NH4Cl was recovered, what was the percent yield? e) How many grams of a the limiting reagent must be used to isolate 10.20 g of C6H5NH2? Assume this is a separate experiment than the one described above. Also assume a purity of 92% for chlorobenzene and the same percent yield.