Answered: What is the percent yield when 49.3 g…

What is the percent yield when 49.3 g of CO2 are formed from the reaction of 0.50 moles of C8H18 with 5.0 moles of O2? 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

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 4.30PAE: 4.30 Copper reacts with nitric acid via the following equation: 3Cu(s)+8HNO3(aq)3Cu(...

See similar textbooks

Related questions

Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.6 mol of NO₂ were…

A: Nitrogen monoxide reacts with oxygen to form nitrogen dioxide. The balanced equation is as follows:…

Q: Calculate the percent yield for the following reaction if 76.8 g of H2O reacted and 125 g of NO were…

A: The mole to mole ratio for H2O and NO in the given reaction is 1:1. Therefore, 18 g of water will…

Q: Calculate the percent yield of sodium sulfate when 32.18 g of sulfuric acid reacts with excess…

A: Percent yield = (actual yield/theoretical yield) × 100% Actual yield of Na2SO4 = 37.91 g (given)…

Q: How many grams of NO are produced when 14.5 g of NH3 are reacted with 12.2 g of O2 according to the…

A: Limiting Reactant is the reactant which is completely consumed during the reaction.

Q: Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with…

A: Given:Moles of C8H18 = 4.000 moles.Moles of O2 = 4.000 moles.actual yield of CO2 = 28.16 g2C8H18 +…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

A: In the given chemical equation, 5.0 mol of O2 completely reacts with 10.0 mol of NO but only 7.0 mol…

Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.5 mol of NO₂ were…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Percent yield = actual yield / theoretical yield x 100%.

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

A: The percent yield of a reaction is calculated by using the following expression: % yield = (Actual…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

A: Record the given data: The given reaction is, Moles of NO = 7.0 mol Moles of O2 = 5.0 mol Moles of…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates…

A: The reaction given in the question is as follows- 2 NO (g) + O2 (g) → 2 NO2 (g) The number of moles…

Q: When 50.0 g of acetylene is allowed to react with excess oxygen, 75.0 g of CO2 are formed. WWhat is…

A: Interpretation- To determine the percentage yield of carbon dioxide when 50 g of acetylene is…

Q: How many moles of O2 would be required to generate 13.0 mol of NO2 in the reaction below assuming…

A: The balanced reaction taking place is given as, => 2 NO (g) + O2 (g) -------> 2 NO2 (g)…

Q: If 10.0 moles of O2 are reacted with excess NO in the reaction below, and only 3.9 mol of NO2 were…

A: For the reaction: O2 (g)+ 2NO (g)→ 2NO2 (g) 1 mol 2 mol 2 mol Given moles of O2 =10 mol…

Q: How many grams of NO are produced when 14.5 g of NH3 are reacted with 12.2 g of O2 according to the…

Q: What is the percent yield if 108 mg SO2 is isolated from the combustion of 82.7 mg of carbon…

A: The percent yield is the ratio of the actual yield to the theoretical yield, an it is expressed as a…

Q: Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of…

A: Combustion of butane (C4H10) takes place as follows: 2C4H10(g)+ 13 O2(g) →8CO2(g)+10H2O(g) By the…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

A: Given: The given reaction is, Moles of NO = 7.0 mol Moles of O2 = 5.0 mol Moles of NO2(actual…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Balanced chemical equation is as follows: It is given that 84.9% of the theoretical yield is equal…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates…

A: Given, 2 NO + O2 ---> 2 NO2 Moles of NO = 7.0 mol Moles of O2 = 5.0 mol

Q: What is the percent yield for a process in which 10.4 g of CH3OH reacts and 10.1 g of CO2 is formed…

A: To solve this problem we will use the given chemical equation to calculate the theoretical yield and…

Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.3 mol of NO₂ were…

Q: how many grams of nitrogen dioxide will be formed

A: Balanced chemical equation: 2NO(g)+O2(g)= 2NO2(g)

Q: If 10.0 moles of O_{2} are reacted with excess NO in the reaction below, and only 4.9 mol of N*O_{2}…

A: Given data: The moles of O2 reacted= 10.0 mole. The moles of NO2 obtained=4.9 mol. Given reaction: 2…

Q: Oxygen can be produced from the catalytic decomposition of KClO3 as shown in the balanced equation…

Q: theoretical yield

Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.2 mol of NO₂ were…

A: The balanced chemical equation between nitrogen oxide and oxygen and its theoretical yield are…

Q: What is the percent yield if 119.30 g O2 reacts with excess NH3 according to the balanced equation…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates…

A: Nitrogen monoxide reacts with oxygen to form nitrogen dioxide. The equation for the balanced…

Q: When HgO is heated, it decomposes into elemental mercury and molecular oxygen. If 10.0 g of Hg is…

Q: How many moles of O2 would be required to generate 13.0 mol of NO in the reaction below assuming the…

A: The given reaction is, Actual mass of NO2 formed is calculated as follows,

Q: n the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O₂ are reacted together. The reaction generates…

A: Given that: 2NO(g) + O2(g) .....> 2NO2(g) Moles pf NO = 7.0Mol Moles of O2 = 5.0moles Moles of…

Q: If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.2 mol of NO₂ were…

A: GIVEN: Reaction: 2 NO (g) + O₂ (g) → 2 NO₂ (g) To Solve: percent yield for the reaction=?

Q: How many moles of NO can be produced by the reaction of 65.00 g of NH3 with 150.0 g of O2 according…

A: Calculate the number of moles of ammonia and oxygen gas.

Q: When 36.7g dimethyl ether (C2H6O) is burned, 58.3g of CO2 is produced. What is the percent yield of…

A: Given, Mass of dimethyl ether burned = 36.7g. Mass of carbon dioxide produced = 58.3g. The…

Q: What is the mass in grams of NO that can be formed from 2.16 moles of NO₂ in the reaction below? 3…

A: In the reaction; 3 NO₂ (g) + H₂O (g) → 2 HNO₃ (g) + NO (g)

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: The considered reaction is, 2 NO (g) + O2 (g)→2NO2 (g)

Q: How many moles of nitrogen gas would be produced if 3.24 moles of copper(II) oxide were reacted with…

A: The given reaction is: 2 NH₃(g) + 3 CuO (s) → 3 Cu(s) + N₂(g) + 3 H₂O(g)

Q: What is the percent yield in a reaction between 8.14 g of N2(g) and 1.48 g of H2(g) in which 3.68 g…

A: The limiting reactant in the given reaction is determined as,

Q: If 225 g of carbon reacts with excess sulfur dioxide to produce 195 g of carbon disulfide, what is…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: To solve this problem first we calculate theoretical yield of NO2 Then we calculate the number of…

Q: Calculate the percent yield for the following reaction if 233 g of NO2 reacted and 175 g of HNO3…

A: The reaction is 3NO2+H2O-----------> 2HNO3+NO Now let us calculate the theoretical yeild of HNO3…

Q: What is the % yield of this reaction when 200.0 g of phosphorus trichloride reacts with excess water…

A: What is the % yield of this reaction when 200.0 g of phosphorus trichloride reacts with excess water…

Q: Ethyl alcohol is prepared industrially by the reaction of ethylene, C2H4, with water. What is the…

Q: If 10.0 moles of O₂ are reacted

A: Given reaction is 2 NO (g) + O₂ (g) →…

Q: If 10.0 moles of O: are reacted with excess NO in the reaction below, and only 5.5 mol of NO2 were…

A: The given reaction is as follows: 2NO(g) + O2(g)------->2NO2(g) The moles of O2 reacting, = 10…

Question

What is the percent yield when 49.3 g of CO₂ are formed from the reaction of 0.50 moles of C₈H₁₈ with 5.0 moles of O₂?

2 C₈H₁₈(l) + 25 O₂(g) → 16 CO₂(g) + 18 H₂O(g)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
Quicklime, CaO, is formed when calcium hydroxide is heated. Ca(OH)2(s) → CaO(s) + H2O(ℓ) The theoretical yield is 65.5 g but only 36.7 g quicklime I is produced. Calculate the percent yield.
Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2 mol NO, calculate how many moles and how many grams of O2 are required for complete reaction. Calculate what mass of NO2, in grams, is produced.
Ammonia gas can be prepared by the following reaction: CaO(s) + 2 NH4Cl(s) 2 NH3(g) + H2O(g) + CaCl2(s) If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g (Study Question 12). If only 16.3 g of NH3 is actually obtained, what is its percent yield?
4.12 In petroleum refining, hydrocarbons are often manipulated by reacting them with H2(g). If hexene, C6H12, is reacted with hydrogen to form hexane, C6H14, how many moles of hydrogen are needed to react with 453 moles of hexene?
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?
ATOM ECONOMY: Benzene, C6H6, is a common compound, and it can be oxidized to give maleic anhydride, C4H2O3, which is used in turn to make other important compounds. (a) What is the % atom economy for the synthesis of maleic anhydride from benzene by this reaction? (b) If 972 g of maleic anhydride is produced from exactly 1.00 kg of benzene, what is the percent yield of the anhydride? What mass of the by-product CO2 is also produced?
Ethylene oxide, C2H4O, is made by the oxidation of ethylene, C2H4. 2C2H4(g)+O2(g)2C2H4O(g) Ethylene oxide is used to make ethylene glycol for automobile antifreeze. In a pilot study, 10.6 g of ethylene gave 9.91 g of ethylene oxide. What is the percentage yield of ethylene oxide?
4.30 Copper reacts with nitric acid via the following equation: 3Cu(s)+8HNO3(aq)3Cu( NO3)2(aq)+2NO(g)+4H2O(l) What mass of NO(g) can be formed when 10.0 g of Cu reacts with 115 g of HNO3?
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
For the chemical reaction Sb2S3+6HCl2SbCl3+3H2S write the conversion factor that would be needed to do each of the following one-step conversions. a. Moles of SbCl3 to moles of H2S b. Moles of Sb2S3 to moles of HCl c. Moles of H2S to moles of HCl d. Moles of Sb2S3 to moles of SbCl3