▾ 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) 1.869 g H₂ Submit Completed ▾ Part D Previous Answers How many molecules (not moles) of NH3 are produced from 5.57x10-4 g of H₂? Express your answer numerically as the number of molecules. ► View Available Hint(s) [5] ΑΣΦ Submit ? < molecules
▾ 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) 1.869 g H₂ Submit Completed ▾ Part D Previous Answers How many molecules (not moles) of NH3 are produced from 5.57x10-4 g of H₂? Express your answer numerically as the number of molecules. ► View Available Hint(s) [5] ΑΣΦ Submit ? < molecules
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
![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
molar
mass
molar
mass
Review | Constants I Periodic Table
Converting between quantities
To convert from a given quantity of one reactant or product to the quantity of another
reactant or product:
. 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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2F003733b2-41d0-45e2-861d-4c00b2709232%2Fh206qw8_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
molar
mass
molar
mass
Review | Constants I Periodic Table
Converting between quantities
To convert from a given quantity of one reactant or product to the quantity of another
reactant or product:
. 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.
![Completed
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)
1.869 g H₂
Submit
Previous Answers
Completed
Part D
Submit
Previous Answers
[5] ΑΣΦ
1
How many molecules (not moles) of NH3 are produced from 5.57x10-4 g of H₂?
Express your answer numerically as the number of molecules.
► View Available Hint(s)
Provide Feedback
?
M Update:
molecules
Next >](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d09ffa2-b6c2-4e97-915d-74d176d987ab%2F003733b2-41d0-45e2-861d-4c00b2709232%2F40z1z3r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Completed
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)
1.869 g H₂
Submit
Previous Answers
Completed
Part D
Submit
Previous Answers
[5] ΑΣΦ
1
How many molecules (not moles) of NH3 are produced from 5.57x10-4 g of H₂?
Express your answer numerically as the number of molecules.
► View Available Hint(s)
Provide Feedback
?
M Update:
molecules
Next >
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