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
100%
How do I find the last part for D
![[Review Topics]
This question has multiple parts. Work all the parts to get the most points.
Aluminum chloride, AlCl3, is made by treating scrap aluminum with chlorine.
2 Al(s) + 3 Cl₂(g) → 2 AlCl3 (8)
If you begin with 2.70 g of
Al and 4.96 g of
Cl₂,
F2
a which reactant is limiting?
Cl₂
Drag and drop your selection from the following list to complete the answer:
Al
AIC13
2.70 g Al x
1. Calculate the amounts of each reactant.
2. Compare the ratio of reactants amounts to the stoichiometric ratio defined by the equation.
4.96 g Cl₂ x
1 mol Al
26.98 g
0.100 mol Al
0.0700 mol Cl₂
Cl₂ is the limiting reactant.
80
F3
1 mol Cl₂
70.90 g
=
= 0.100 mol Al
1.43 mol Al
>
1 mol Cl₂
b What mass of AlCl3 can be produced?
Show Hint
Q
= 0.0700 mol Cl₂
F4
2 mol Al
3 mol Cl₂
Cengage Learning | Cengage Technical Support
0
F5
C
Correct
F6
«
F7
[References]
DII
F8
F9
1
F10
<
Email
F11](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbe53d701-6691-4314-9bda-29e504eeb7d9%2F1a7d9c97-e68b-425f-9f59-e6325103508a%2Fuf9wmxr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:[Review Topics]
This question has multiple parts. Work all the parts to get the most points.
Aluminum chloride, AlCl3, is made by treating scrap aluminum with chlorine.
2 Al(s) + 3 Cl₂(g) → 2 AlCl3 (8)
If you begin with 2.70 g of
Al and 4.96 g of
Cl₂,
F2
a which reactant is limiting?
Cl₂
Drag and drop your selection from the following list to complete the answer:
Al
AIC13
2.70 g Al x
1. Calculate the amounts of each reactant.
2. Compare the ratio of reactants amounts to the stoichiometric ratio defined by the equation.
4.96 g Cl₂ x
1 mol Al
26.98 g
0.100 mol Al
0.0700 mol Cl₂
Cl₂ is the limiting reactant.
80
F3
1 mol Cl₂
70.90 g
=
= 0.100 mol Al
1.43 mol Al
>
1 mol Cl₂
b What mass of AlCl3 can be produced?
Show Hint
Q
= 0.0700 mol Cl₂
F4
2 mol Al
3 mol Cl₂
Cengage Learning | Cengage Technical Support
0
F5
C
Correct
F6
«
F7
[References]
DII
F8
F9
1
F10
<
Email
F11
![bwhat mass of AlCl3 can be produced?
Mass= 6.22
g
7.00 x 10-2 mol Cl₂ ×
Calculate the mass of product based on the amount of the limiting reactant.
2 mol AlCl3
3 mol Cla
7.00 x 10-2 mol Cl₂ x
X
133.3 g
1 mol AlCl3
CWhat mass of the excess reactant remains when the reaction is completed?
Mass=1.441
9
Submit
[Review Topics]
d Set up an amounts table for this problem.
Equation
2 Al(s)
Initial amount (mol) 1.00x10^-1
Change (mol)
Show Hint
2.70 g Al available - 1.26 g Al used = 1.44 g Al remains
Determine the mass of the second reactant required in the reaction from the limiting reactant in a similar c
reagent is the difference between its starting mass and what was used in the reaction.
Correct
2 mol Al
26.98 g
X
3 mol Cl₂
= 1.26 g Al used
1 mol Al
6.22 g AIC13
+ 3 Cl₂ (g)
7.00x10^-2
-7.00x10^-2
Correct
→ 2 AlCl3 (s)
0
[References]
Cengage Learning | Cengage Technical Support](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbe53d701-6691-4314-9bda-29e504eeb7d9%2F1a7d9c97-e68b-425f-9f59-e6325103508a%2Fc2pikte_processed.jpeg&w=3840&q=75)
Transcribed Image Text:bwhat mass of AlCl3 can be produced?
Mass= 6.22
g
7.00 x 10-2 mol Cl₂ ×
Calculate the mass of product based on the amount of the limiting reactant.
2 mol AlCl3
3 mol Cla
7.00 x 10-2 mol Cl₂ x
X
133.3 g
1 mol AlCl3
CWhat mass of the excess reactant remains when the reaction is completed?
Mass=1.441
9
Submit
[Review Topics]
d Set up an amounts table for this problem.
Equation
2 Al(s)
Initial amount (mol) 1.00x10^-1
Change (mol)
Show Hint
2.70 g Al available - 1.26 g Al used = 1.44 g Al remains
Determine the mass of the second reactant required in the reaction from the limiting reactant in a similar c
reagent is the difference between its starting mass and what was used in the reaction.
Correct
2 mol Al
26.98 g
X
3 mol Cl₂
= 1.26 g Al used
1 mol Al
6.22 g AIC13
+ 3 Cl₂ (g)
7.00x10^-2
-7.00x10^-2
Correct
→ 2 AlCl3 (s)
0
[References]
Cengage Learning | Cengage Technical Support
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