percent yield of a reaction that produces 265.0 g of Fe when 5.00 moles of Fe,O, react with 5.00 moles of Al according to the following reaction. SHOW YOUR WORK Fe203 (s) + 2 Al (s) Al203 (s) + 2 Fe (s)

percent yield of a reaction that produces 265.0 g of Fe when 5.00 moles of Fe,O, react with 5.00 moles of Al according to the following reaction. SHOW YOUR WORK Fe203 (s) + 2 Al (s) Al203 (s) + 2 Fe (s)

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.77PAE: The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce...

See similar textbooks

Related questions

Q: A container holds 15.0 g of P₄O₆ and 6.00 g of O₂. The following reaction occurs: P₄O₆ + 2O₂ →…

A: In a chemical reaction, the theoretical yield of the product is known according to the chemical…

Q: How many grams of HCl are produced when 16.0 g of CH, react with 71.0 g of Cl, to produce 50.5 g of…

Q: Sulfur dioxide reacts with oxygen to produce sulfur trioxide 150 g of sulfur dioxide is reacted with…

A: 1. The reaction is: 2 SO2 + O2 ---> 2 SO3

Q: Consider the following reaction: 2 Al + 6 HBr → 2 AlBr3 + 3 H2 When 1.61 moles of Al reacts…

A: 2Al + 6HBr → 2AlBr3 + 3H2 2 moles of Al and 6 moles of HBr forms two moles of AlBr3. It simply…

Q: (CH3(CH2),CH,) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide (CO2) and…

Q: Given the reaction Fe + Cl=FeCl3 if 5.00 moles each of Fe and Cl2 reacts, how many grams of FeCl3…

Q: How many grams of KBrO3, 167.0 g/mol, are required to prepare 0.625 moles of Br2 according to the…

Q: 4. Phosphorus pentachloride reacts with water to give phosphoric acid and hydrogen chloride. In one…

Q: Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:…

Q: 3. Octane is one of the hydrocarbon components in gasoline, which is the main fuel source for…

Q: Given the follow ing equation: 2 NaCl03 2 NaCl + 3 02, if 12.00 moles of NaClO3 reacted in the 7.…

A: The balanced chemical equation for the reaction is given below:

Q: Carbon tetrachloride (CC14) can be produced using the following reaction. If enough carbon and…

A: Percent yield is defined as the percentage ratio of the actual yield to the theoretical yield…

Q: How many grams of KBrO3, 167.0 g/mol, are required to prepare 0.957 moles of Br2 according to the…

A: Given information: Molar mass of KBrO3 is 167.0 g/mol. Moles of Br2 is 0.957 moles The given…

Q: Given the following equation 2 H2 + O2 --> 2 H2O If 4.0 mol of H2 reacted, how many moles…

Q: student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr. C6H6 +…

A: To solve this problem first we have to calculate the theoretical yield using the balanced chemical…

Q: enO MH 8N Homework • Unanswered Magnesium oxide and ammonium bromide react to produce ammonia gas…

A: Magnesium oxide and ammonium bromide react to produce ammonia gas, water and magnesium bromide.…

Q: Plants use photosynthesis to change carbon dioxide and water into glucose and oxygen, as shown in…

Q: Aluminum carbide reacts with water to produce methane and aluminum hydroxide in the reaction shown…

Q: You react 100.0 g of O2 and 50.0 g of H2 in a container and produce water. 2H2 + O2 → 2H2O How…

A: Limiting reactant :- reactant which is present in less amount than required as per balanced chemical…

Q: 1. Use the following equation to solve the problem below: 3 SiO, + 4 Al → 3 Si + 2 Al,O, a. If 6.0…

Q: How many grams of SO3 are produced when 20.0 g FeS2 react with 16.0 g O2 according to this balanced…

A: The answer to the following question is- Reaction : 4 FeS2 + 15 O2 -----> 2 Fe2O3 + 8 SO3

Q: COG 2) When 10.0 g of Aluminum is allowed to react with 35.0 g of chlorine gas to produce aluminum…

A: The given reaction is 2Al + 3Cl2 = 2AlCl3 The given mass of Al and chlorine are converted into…

Q: Sodium chloride (NaCl) reacts with fluorine gas (F2) to produce sodium fluoride (NaF) and chlorine…

A: The reaction taking place will be 2 NaCl + F2 -------> 2 NaF + Cl2 hence from the above…

Q: Gaseous butane (CH;(CH)¸CH;) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide…

Q: The decomposition of solid aluminum oxide results in the production of solid aluminum and molecular…

Q: In a particular reaction 5.00 moles of NH3 were produced. How many moles of H2 and how many moles of…

A: Nitrogen reacts with hydrogen to form ammonia. The equation for the balanced chemical reaction is…

Q: The depletion of ozone (O3) in the stratosphere has been a matter of great concern among scientists…

Q: 1. When carbon disulfide burns in the presence of oxygen, sulfur dioxide and carbon dioxide are…

Q: The steel-making process described in the Transition Metal section of the Elements Handbook shows…

A: When two reactive compounds are mixed, then they react according to the stoichiometry of the…

Q: When powdered zinc is heated with sulfur, a violent reac-tion occurs, and zinc sulfide forms:Zn(s)…

A: The answer for subpart a is given below. Kindly repost the subpart b) as separate question Given:…

Q: Solid sodium reacts violently with water producing heat, hydrogen gas and sodium hy- droxide. How…

A: Balanced Reaction 2Na(s) + 2 H2 O(l) ---> 2 NaOH(aq) + H2 (g) Mass of sodium = 65.4 g Atomic mass…

Q: Given the unbalanced equation H2SO4 + NaOH --------> Na2SO4 + H2O a. How many moles of NaOH will…

A: (a)The given balanced reaction is,

Q: How many mols of calcium chloride are produced if 0.112 mol of calcium reacts? Ca(s) + Cl2(g) ->…

Q: C2H6 + Cl2 C2H5Cl + "Other Stuff" The formation of these other products reduces the yield of…

Q: Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:…

A: Given: Mass of Al = 16.0 g Mass of Cl2 = 21.0 g Molar mass of Cl2 = 70.906 g/mol Excess reagent: Al…

Q: Given the reaction: 2AI + 3Cl2 +2AICI3 How many moles of aluminum chloride is formed if 4.5 moles of…

A: Balanced chemical Equation 2Al+ 3 Cl2 → 2AlCl3 According to this balanced…

Q: C2H6 + Cl2 C2H5Cl + "Other Stuff" The formation of these other products reduces the yield of…

A: 1 C2H6 + 1 Cl2 -> 1 C2Cl5 + 1 HCl 200 g 240 g 168 g Molar…

Q: Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and…

A: Answer: The percentage yield of water is 81.48 % or 81%{up to two significant figure}

Q: When ethane, C2H6, reacts with chlorine, Cl2, the main product is C2H5Cl, but other products…

A: The required reaction is given below.

Q: Ethyl alcohol burns, producing carbon dioxide and water: C2H5OH +302 2CO2+3 H20 (a) If 2.5 mol of…

A: a. From the reaction it is clear that 1 mole ethanol reacts with 3 moles oxygen to give 2 moles CO2…

Q: More Than Enough Directions: Read carefully the following problems. Find what is asked for each…

Q: Ammonia is produced by the reaction of hydrogen and nitrogen as follows N2(g)+3H2(g)→2NH3(g) ammonia…

A: • Theoritical yield can be calculated by the help of stichimetric coefficient of reactant.• No of…

Q: Pentane (C5H12) undergoes complete combustion in the presence of excess oxygen gas as shown in the…

A: The number of moles of carbon dioxide formed is given below

Q: Glucose, C6H12O6 is used as an energy source by the human body. The overall reaction in the body is…

A: Solution Optically active polyhydroxy aldehydes (aldcses) or ketones (ketoses) or compounds that on…

Q: C5H12 +8 02-5 cO2 + 6 H20 Using the balanced chemical equation above, calculate the number of moles…

Q: Reaction Stoichiometry Given the following reaction: 5Fe+ 3O2 ---> Fe3O4+ 2FeO a. How many moles…

A: The number of moles is determined as the mass of a substance upon its molar mass.

Q: + O2 → FE2O3 How many moles of FeżO3 are produced when 0.265 moles of Fe are reacted? 4. Using the…

A: Given, Moles of Fe atom is 0.265 mol. Required, moles of Fe2O3

Q: Consider the reaction for the combustion of octane (Cs H18). 2C H18 +2502 16CO2 + 18H2O Part A How…

A: A) The given reaction for the combustion of octane is, 2C8H18 + 25O2 ---> 16CO2 + 18H2O From the…

Q: A chemist uses carbon, CaO, HCl and H₂O for C₆H₄Cl₂ (147.09 g mol⁻¹). Assuming that the efficiency…

Q: C3H8 + 5O2 → 3CO2 + 4 H2O, with the given equation, thirty (30) grams of C3H8 burns in air to…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Determine the percent yield of a reaction that produces 265.0 g of Fe when 5.00
moles of Fe,O, react with 5.00 moles of Al according to the following reaction.
SHOW YOUR WORK
Fe2O3 (s) + 2 Al (s)
Al2O3 (s) + 2 Fe (s)
Paragraph
BIU
KA
</> EQ
Record Video
Record Audio
Add a File
MacBook Air

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

Steps to calculate percent yield

Limiting reagent

Theoretical yield

Percent yield

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
For the following reaction: C3H8(g) + O2(g) ------> CO2(g) + H2O(g) Q: Calculate the theoretical yield of CO2(g) in gram
A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)
The hydrated salt, MY3·xH2O, was heated strongly in a crucible to remove all the watermolecules of crystallization.The data are for this experiment are given in the table below.Mass of empty crucible and cover 29.73 gMass of crucible, cover, and hydrated salt 32.72 gMass of crucible, cover, and anhydrous salt 31.52 gMolar mass of anhydrous salt 241.88 g/mol(i) Calculate the % composition by mass of water in the hydrated salt.(ii) Determine the value of x.(iii) M is in Period 4 of the Periodic Table of the Elements.If Y = NO3–, identify the element M.(iv) What is the name of this hydrated salt? ___
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2Sa. Find the Mass to Mass Stoichiometry Calculation b. Upon solving A, find the LIMITING REAGENT, EXCESS REAGENT and the AMOUNT IN EXCESSc. Find the Percentage Yield from Problem Ad. Find the number of dosage form and packaging that can be produced from the stoichiometric calculation based on Problem A
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2Sa. Find the Mass to Mass Stoichiometry Calculation b. Upon solving A, find the LIMITING REAGENT, EXCESS REAGENT and the AMOUNT IN EXCESSc. Find the Percentage Yield from Problem A
Potassium chromate, a bright yellow solid, is produced by the reaction of solid chromium ore (FeCr2O4) with solid potassium carbonate and gaseous oxygen at high temperatures. The other products of the reaction are solid iron (III) oxide and gaseous carbon dioxide. If you use 169.0g of chromium ore, 298.0g of potassium carbonate and 75.00g of oxygen in a sealed reaction vessel, what is the limiting reagent? Give the theoretical yield of potassium chromate, in grams, for each one.