How Do You Calculate Percent Yield of C2H5Cl in a Complex Reaction?

  • Thread starter Thread starter alingy1
  • Start date Start date
  • Tags Tags
    Chemical
Click For Summary

Discussion Overview

The discussion revolves around calculating the percent yield of C2H5Cl in a complex reaction involving ethane and chlorine gas. Participants explore the implications of minor products on yield calculations and the assumptions underlying theoretical yield in chemical reactions.

Discussion Character

  • Homework-related, Debate/contested, Conceptual clarification

Main Points Raised

  • One participant presents a homework problem involving the reaction of ethane with chlorine, noting that the solution manual provides a percent yield of 82.9% based on a simplified reaction equation.
  • Another participant argues that the presence of minor products should impact the yield calculations, questioning the validity of the simplified equation used in the solution manual.
  • A different participant asserts that the other products may not necessarily affect the calculations, suggesting they could be unreacted starting materials instead.
  • One participant explains that theoretical yield calculations typically assume only one main product, highlighting the challenge of balancing reactions with multiple products.
  • Another participant acknowledges that multiple balanced equations could be correct, raising questions about the applicability of theoretical yield when multiple products are present.
  • Clarification is provided that HCl is not considered a separate product in this context, as its formation is directly related to the main product, C2H5Cl.

Areas of Agreement / Disagreement

Participants express disagreement regarding the impact of minor products on yield calculations and the validity of the simplified reaction equation. The discussion remains unresolved, with multiple competing views on the assumptions of theoretical yield.

Contextual Notes

Participants note limitations in balancing reactions with multiple products and the assumptions made in theoretical yield calculations. The discussion reflects uncertainty regarding the role of minor products and unreacted materials in yield assessments.

alingy1
Messages
325
Reaction score
0

Homework Statement




"The reaction of ethane gas (C2H6) with chlorine gas produces C2H5Cl as its main product (along with HCl). In addition, the reaction invariably produces a variety of other minor products, including C2H4Cl2, C2H3Cl3, and others. Naturally, the pro- duction of these minor products reduces the yield of the main product. Calculate the percent yield of C2H5Cl if the reaction of 300. g of ethane with 650. g of chlorine produced 490. g of C2H5Cl." (Zumdahl, Chemistry, 2013)

Homework Equations



Balancing and math principles.

The Attempt at a Solution



Ok, I have the answer in the solution manual. It gives out 82.9%.
But, the thing I do not understand about the way they do the problem is this:
They use the formula C2H6+ Cl2-> C2H5Cl+ HCl
However, that's not what is really happening. There are other products formed.
I thought of this formula (which is missing ''the other'' products):
C2H6+ Cl2-> C2H5Cl+ HCl +C2H4Cl2+C2H3Cl3 + others
I found different ways of balancing this last formula if I ignore the others.

Why does the first equation give the right answer? Won't the other molecules intervene in the calculations?
 
Physics news on Phys.org
No, they don't. You can't be certain the other products were produced anyway. The other "products" COULD be unreacted starting material!
 
But, there still may be other products. I don't understand how those cannot have an impact on the reaction balancing.
 
Theoretical yield assumes only one product.

Note that in this particular case you can't uniquely balance reaction with several products. Each of these:

2C2H6 + 3Cl2 -> C2H5Cl + C2H4Cl2 + 3HCl

50C2H6 + 67Cl2 -> 33C2H5Cl + 17C2H4Cl2 + 67HCl

1028C2H6 + 1119Cl2 -> 937C2H5Cl + 91C2H4Cl2 + 1119HCl

is balanced OK. Which one of these is the correct one?
 
All of them could be correct i guess. Hmm, you are intriguing me here. Theoretical yield applies only when there is one product? What about the HCl?
 
Sorry, lousy wording, one main product. HCl doesn't matter, as its amount is related to the main product - you don't need more ethane to produce HCl.
 

Similar threads

Percentage yield in a reaction problem
  • · Replies 4 ·
Replies
4
Views
3K
Chemistry How do we interpret the steps in the algorithm to balance a redox equation?
  • · Replies 7 ·
Replies
7
Views
3K
Calculating Percent Yield of PbI2 in 2CsI + Pb(NO3)2 Reaction
  • · Replies 7 ·
Replies
7
Views
3K
Calculating Mass Percent of Aluminum in a Sample Using Ideal Gas Law
  • · Replies 5 ·
Replies
5
Views
2K
What Is the Percent Yield of Al2O3 in This Reaction?
  • · Replies 4 ·
Replies
4
Views
7K
How Do You Calculate Equilibrium Concentrations in a Redox Reaction?
  • · Replies 2 ·
Replies
2
Views
4K
What Are the Identities of Compounds Y and Z in This Boron Isolation Reaction?
  • · Replies 1 ·
Replies
1
Views
3K
Lab Calculations: How to Find Theoretical Yield
  • · Replies 1 ·
Replies
1
Views
4K
How do you find the product of a chemical reaction?
  • · Replies 9 ·
Replies
9
Views
6K
How Do You Calculate the Formation Reaction ΔH Using Hess's Law?
  • · Replies 1 ·
Replies
1
Views
5K