D. Determine the percentage yield of the reaction; E. Calculate the percent error and F. Compute for the excess amount of the excess reactant if applicable;
D. Determine the percentage yield of the reaction; E. Calculate the percent error and F. Compute for the excess amount of the excess reactant if applicable;
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...
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Question
Answer letter D, E and F only.
ll. Direction: Carefully read the following problems
Do the following :
A. Balance the chemical equation
B. Identify the limiting reactant and the excess reactant if applicable;
C. Compute for the theoretical yield;
D. Determine the percentage yield of the reaction;
E. Calculate the percent error and
F. Compute for the excess amount of the excess reactant if applicable;
![3. Fifty grams of Chlorine reacts completely with Phosphorus obtaining ninety grams of the
product.
P +C12,
PCI.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba541c68-e096-4d43-9609-0fd5ded505f6%2Feae57448-6b6f-44e6-ae79-23ea160c663f%2Fg7zc1uo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. Fifty grams of Chlorine reacts completely with Phosphorus obtaining ninety grams of the
product.
P +C12,
PCI.
![Step 2
Recall the reaction,
P + Cl
PCI3
----->
mass of Cl2 = 50g,
molar mass of Cl2=70.90 g mol1
mass of PCI3 = 90 g
Molar mass of PC|3= 137.33 g mol--
Step 3
A) Reaction,
P + Cl2
PCI3
----->
Balanced reaction,
2P + 3C12
-----> 2PCI3
B) In this question, only mass of Cl2 is given so Cl2 act as limiting reagent because it is completely
consumed and P act as excess reagent.
Step 4
C)From Balanced reaction,
2P + 3C12
-> 2PCI3
----->
3x70.90 g of Cl2 produced 2x137.33 g of PCI3
=> 1 g of Cl2 produced = 1.29 g of PCI3
so,
50 g of Cl2 produced = 50x1.29 g of PCI3
d - CAC](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba541c68-e096-4d43-9609-0fd5ded505f6%2Feae57448-6b6f-44e6-ae79-23ea160c663f%2Farzvbus_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Step 2
Recall the reaction,
P + Cl
PCI3
----->
mass of Cl2 = 50g,
molar mass of Cl2=70.90 g mol1
mass of PCI3 = 90 g
Molar mass of PC|3= 137.33 g mol--
Step 3
A) Reaction,
P + Cl2
PCI3
----->
Balanced reaction,
2P + 3C12
-----> 2PCI3
B) In this question, only mass of Cl2 is given so Cl2 act as limiting reagent because it is completely
consumed and P act as excess reagent.
Step 4
C)From Balanced reaction,
2P + 3C12
-> 2PCI3
----->
3x70.90 g of Cl2 produced 2x137.33 g of PCI3
=> 1 g of Cl2 produced = 1.29 g of PCI3
so,
50 g of Cl2 produced = 50x1.29 g of PCI3
d - CAC
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