▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. ► View Available Hint(s) VE ΑΣΦ Submit Part C VE ΑΣΦ ? How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) Submit g NH3 ? g H₂
▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. ► View Available Hint(s) VE ΑΣΦ Submit Part C VE ΑΣΦ ? How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) Submit g NH3 ? g H₂
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
Answer part A,B, and C
![▼
Part B
How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂.
Express your answer numerically in grams.
View Available Hint(s)
VE ΑΣΦ
Submit
Part C
How many grams of H₂ are needed to produce 10.59 g of NH3?
Express your answer numerically in grams.
► View Available Hint(s)
5 ΑΣΦ
g NH3
Submit
g H₂](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2Fff01b330-21f8-43c9-b7e4-4f9d4f8f36cd%2Finzbjza_processed.jpeg&w=3840&q=75)
Transcribed Image Text:▼
Part B
How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂.
Express your answer numerically in grams.
View Available Hint(s)
VE ΑΣΦ
Submit
Part C
How many grams of H₂ are needed to produce 10.59 g of NH3?
Express your answer numerically in grams.
► View Available Hint(s)
5 ΑΣΦ
g NH3
Submit
g H₂
![Learning Goal:
To understand how to use stoichiometry to convert between quantities of reactants and
products in chemical equations.
Stoichiometry describes the quantitative relationships among the reactants and
products of a balanced reaction by directly comparing mole ratios. Stoichiometry can
be used to convert mass, number of moles, or number of particles between products
and reactants, as shown in the flowchart displayed in the figure.
Substance A
Substance B
number of
particles
Avogadro's
number
Avogadro's
number
number of
particles
I
I
mass
moles
coefficients from balanced
chemical equation
moles
mass
I
molar
mass
molar
mass
Converting between quantities
To convert from a given quantity of one reactant or product to the quantity of another
reactant or product:
Review | Constants I Periodic Table
. First, convert the given quantity to moles. Use molar masses to convert
masses to moles, and use Avogadro's number (6.02 x 1023 particles per
mole) to convert number of particles to moles.
• Next, convert moles of the given reactant or product to moles of the desired
reactant or product using the coefficients of the balanced chemical equation.
For example, in the chemical equation
2H2 + O2
2H₂O
the coefficients tell us that 2 mol of H₂ reacts with 1 mol of O₂ to produce
2 mol of H₂O.
▼
• Finally, convert moles of the desired reactant or product back to the desired
units. Again, use molar masses to convert from moles to masses, and use
Avogadro's number to convert from moles to number of particles.
Reaction of hydrogen and nitrogen to form ammonia
Hydrogen gas, H2, reacts with nitrogen gas, N₂, to form ammonia gas, NH3, according
to the equation
3H2(g) + N2(g) →→2NH3(g)
NOTE: Throughout this tutorial use molar masses expressed to five significant figures.
Part A
How many moles of NH3 can be produced from 15.0 mol of H₂ and excess N₂?
Express your answer numerically in moles.
►View Available Hint(s)
|VLI ΑΣΦ 4
?
mol NH3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2Fff01b330-21f8-43c9-b7e4-4f9d4f8f36cd%2F3y904l9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Learning Goal:
To understand how to use stoichiometry to convert between quantities of reactants and
products in chemical equations.
Stoichiometry describes the quantitative relationships among the reactants and
products of a balanced reaction by directly comparing mole ratios. Stoichiometry can
be used to convert mass, number of moles, or number of particles between products
and reactants, as shown in the flowchart displayed in the figure.
Substance A
Substance B
number of
particles
Avogadro's
number
Avogadro's
number
number of
particles
I
I
mass
moles
coefficients from balanced
chemical equation
moles
mass
I
molar
mass
molar
mass
Converting between quantities
To convert from a given quantity of one reactant or product to the quantity of another
reactant or product:
Review | Constants I Periodic Table
. First, convert the given quantity to moles. Use molar masses to convert
masses to moles, and use Avogadro's number (6.02 x 1023 particles per
mole) to convert number of particles to moles.
• Next, convert moles of the given reactant or product to moles of the desired
reactant or product using the coefficients of the balanced chemical equation.
For example, in the chemical equation
2H2 + O2
2H₂O
the coefficients tell us that 2 mol of H₂ reacts with 1 mol of O₂ to produce
2 mol of H₂O.
▼
• Finally, convert moles of the desired reactant or product back to the desired
units. Again, use molar masses to convert from moles to masses, and use
Avogadro's number to convert from moles to number of particles.
Reaction of hydrogen and nitrogen to form ammonia
Hydrogen gas, H2, reacts with nitrogen gas, N₂, to form ammonia gas, NH3, according
to the equation
3H2(g) + N2(g) →→2NH3(g)
NOTE: Throughout this tutorial use molar masses expressed to five significant figures.
Part A
How many moles of NH3 can be produced from 15.0 mol of H₂ and excess N₂?
Express your answer numerically in moles.
►View Available Hint(s)
|VLI ΑΣΦ 4
?
mol NH3
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 5 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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.Recommended textbooks for you
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY