3. Aluminum does not occur naturally in its elemental form and therefore must be refined fromore. Part of this process involves the balanced reaction shown here.2 Al2O3 + 3 C4 Al + 3 CO2A production run utilizes 25.0 kg Al2O3 and 5.00 kg of carbon, and produces 9.47 kg of Al.a. Calculate the molar mass of Al2O3 (show your work here):b. Calculate the theoretical yield of Al in moles. This will require two stoichiometrycalculations - one for each reactant. Show all work clearly.c. Limiting reactant:Excess reactant:d. Convert the theoretical yield (from part b) into kg of Al.Calculate the percent yield of thisprocess.

Answered: 3. Aluminum does not occur naturally in…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 36QAP

See similar textbooks

Similar questions

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.
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
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.
What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?
The aspirin substitute, acetaminophen (C8H9O2N), is produced by the following three-step synthesis: I.C6H5O3(s)+3H2(g)+HCl(aq)C6H8ONCl(s)+2H2O(l)II.C6H8ONCl(s)+NaOH(aq)C6H7ON(s)+H2O(l)+Nacl(aq)III.C6H7ON(s)+C4H6O3(l)C8H9O2N(s)+HC2H3O2(l) The first two reactions have percent yields of 87% and 98% by mass, respectively. The overall reaction yields 3 moles of acetaminophen product for every 4 moles of C6H5O3N reacted. a. What is the percent yield by mass for the overall process? b. What is the percent yield by mass of Step III?
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.
You know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to determine the amount of product that will be produced? Explain.
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
3.18 Diborane and related compounds were proposed as rocket fuels in the 1950s. A representative reaction for this class of molecules is that of B2H6 and O2 to form B2O3 and H2O. Write the balanced chemical equation for this process.
What is the theoretical yield for a reaction, and how does this quantity depend on the limiting reactant?
3.84 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4, and oxygen, O2. (a) Draw the resulting state after this set of re- actants has reacted as far as possible. (b) Use the drawings to explain the stoichiometry represented in the balanced chemical equation for the combustion of methane.

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

SEE MORE TEXTBOOKS