Homework Help is Here – Start Your Trial Now!
Science
Chemistry
a What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10 g N2 and 5.60 x 102 g H2? Mass = 1216.01 The strategy we will generally use to solve limiting reactant problems is to assume each reactant is limiting, and then calculate the quantity of product each reactant could produce if it were limiting. The reactant that produces the smallest quantity of product is the limiting reactant (runs out first) and therefore determines the mass of product that can be produced. Assuming N2 is limiting: 1 mol N2 28.02 g N2 17.03 g NH3 2 mol NH3 x mol N2 1.00 x 10° g N2 × mol NH3 = 1.22 x 103 g NH3 Assuming H2 is limiting: 1 mol H2 2.016 g H2 2 mol NH3 17.03 g NH3 mol NH3 5.60 x 10° g H, × 3 mol H2 = 3.15 x 103 g NH, Because N2 produces the smaller mass of product (1220 g vs. 3150 g NH3), N2 is limiting and 1220 g NH3 can be produced. As soon as 1220 g of NH3 is produced, all of the N2 has run out. Even though we have enough H2 to produce more product, there is no more N2 present as soon as 1220 g of NH3 have been produced. b What mass of which starting material would remain unreacted? g of nitrogen v would remain unreacted.

a What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10 g N2 and 5.60 x 102 g H2? Mass = 1216.01 The strategy we will generally use to solve limiting reactant problems is to assume each reactant is limiting, and then calculate the quantity of product each reactant could produce if it were limiting. The reactant that produces the smallest quantity of product is the limiting reactant (runs out first) and therefore determines the mass of product that can be produced. Assuming N2 is limiting: 1 mol N2 28.02 g N2 17.03 g NH3 2 mol NH3 x mol N2 1.00 x 10° g N2 × mol NH3 = 1.22 x 103 g NH3 Assuming H2 is limiting: 1 mol H2 2.016 g H2 2 mol NH3 17.03 g NH3 mol NH3 5.60 x 10° g H, × 3 mol H2 = 3.15 x 103 g NH, Because N2 produces the smaller mass of product (1220 g vs. 3150 g NH3), N2 is limiting and 1220 g NH3 can be produced. As soon as 1220 g of NH3 is produced, all of the N2 has run out. Even though we have enough H2 to produce more product, there is no more N2 present as soon as 1220 g of NH3 have been produced. b What mass of which starting material would remain unreacted? g of nitrogen v would remain unreacted.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 139QRT
See similar textbooks
icon
Related questions
Question
a What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10° g N2 and 5.60 x 102 g H2? Mass = 1216.01 The strategy we will generally use to solve limiting reactant problems is to assume each reactant is limiting, and then calculate the quantity of product each reactant could produce if it were limiting. The reactant that produces the smallest quantity of product is the limiting reactant (runs out first) and therefore determines the mass of product that can be produced. Assuming N2 is limiting: 1 mol N2 28.02 g N2 2 mol NH3 17.03 g NH3 mol NH3 1.00 × 10° g N, × mol N2 = 1.22 x 103 g NH, Assuming H2 is limiting: 17.03 g NH3 1 mol H2 2.016 g H2 2 mol NH3 5.60 x 10° g H, х 3 mol H2 mol NH3 = 3.15 x 10° g NH3 Because N2 produces the smaller mass of product (1220 g vs. 3150 g NH3), N2 is limiting and 1220 g NH3 can be produced. As soon as 1220 g of NH3 is produced, all of the N2 has run out. Even though we have enough H2 to produce more product, there is no more N2 present as soon as 1220 g of NH3 have been produced. b What mass of which starting material would remain unreacted? g of nitrogen v would remain unreacted. Previous Next
Transcribed Image Text:a What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10° g N2 and 5.60 x 102 g H2? Mass = 1216.01 The strategy we will generally use to solve limiting reactant problems is to assume each reactant is limiting, and then calculate the quantity of product each reactant could produce if it were limiting. The reactant that produces the smallest quantity of product is the limiting reactant (runs out first) and therefore determines the mass of product that can be produced. Assuming N2 is limiting: 1 mol N2 28.02 g N2 2 mol NH3 17.03 g NH3 mol NH3 1.00 × 10° g N, × mol N2 = 1.22 x 103 g NH, Assuming H2 is limiting: 17.03 g NH3 1 mol H2 2.016 g H2 2 mol NH3 5.60 x 10° g H, х 3 mol H2 mol NH3 = 3.15 x 10° g NH3 Because N2 produces the smaller mass of product (1220 g vs. 3150 g NH3), N2 is limiting and 1220 g NH3 can be produced. As soon as 1220 g of NH3 is produced, all of the N2 has run out. Even though we have enough H2 to produce more product, there is no more N2 present as soon as 1220 g of NH3 have been produced. b What mass of which starting material would remain unreacted? g of nitrogen v would remain unreacted. Previous Next
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Stoichiometry
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
Recommended textbooks for you
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS