Solving Limiting Reactions: O2 + 2NO2-->2NO2

  • Thread starter Thread starter megas
  • Start date Start date
  • Tags Tags
    Reactions
Click For Summary

Discussion Overview

The discussion revolves around the concept of limiting reactions in a chemical equation, specifically the reaction involving O2 and NO2. Participants seek to understand how to identify the limiting reagent and calculate the amounts of reactants and products involved. The scope includes theoretical understanding and practical application in chemistry.

Discussion Character

  • Homework-related
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant requests help with a limiting reaction problem involving the equation O2 + 2NO2 --> 2NO2, expressing confusion over the professor's explanation.
  • Another participant suggests that to find the limiting reagent, mole calculations must be performed to determine which reactant is in excess.
  • A different participant points out that the initial chemical equation provided is incorrect, noting discrepancies in the number of atoms on each side.
  • Another participant proposes the corrected reaction as O2 + 2NO --> 2NO2, highlighting the need for accurate representation of the reaction.
  • One participant shares their method of determining the limiting reagent by calculating the yield for each reactant separately, suggesting it is a more efficient approach.
  • Several participants express gratitude for the assistance and clarification provided throughout the discussion.

Areas of Agreement / Disagreement

Participants generally agree on the need to identify the limiting reagent through calculations, but there is disagreement regarding the correct formulation of the chemical reaction, with multiple corrections made to the initial equation.

Contextual Notes

The discussion includes unresolved issues regarding the correct stoichiometry of the reaction, as participants provide differing equations and corrections without reaching a consensus on the correct form.

megas
Messages
13
Reaction score
0
LIMITING reactions(please help me! (is it that hard?)NEED A CHALLENGE?

hi, i was wondering if anyone could help me out with my chemistry 1 stuff. The proffessor isn't explaining it very well to me. so...well, here's the question, i need help with limiting reactions, O2 + 2No2-->2NO2, if they gave me 10.00g of 02, and 20g of 2NO2 what is the amount of 2NO2, the limiting reaction and amount left? i could use the answere, but i would really like to know how to do it thanks
 
Last edited:
Chemistry news on Phys.org
The main problem is that you will have to find which reactant is excess, so the other will be the limiting reagent. To find this, you'll use mole calculations. Which one is excess, 10.00 g of O2 or 20 g of NO2? You can use O=16 and N=14 g/mole.
 
megas said:
hi, i was wondering if anyone could help me out with my chemistry 1 stuff. The proffessor isn't explaining it very well to me. so...well, here's the question, i need help with limiting reactions, O2 + 2No2-->2NO2, if they gave me 10.00g of 02, and 20g of 2NO2 what is the amount of 2NO2, the limiting reaction and amount left? i could use the answere, but i would really like to know how to do it thanks
Make sure the equation you provide is correct. In this case it is not. You have NO2 as a reactant and product.
 
sorry

the right formula is O2 + No2 -> 2No2,.. ok thanks i get it now, lol, (dragonball Z rules) :smile:
 
No, this is incorrect either. Please take a good look at your reaction; on the left, you have three oxygens and one nitrogen, but on the right, you have two nitrogens and four oxygens.

I bet the reaction should be like this:

[tex]O_2 + 2NO \longrightarrow 2NO_2[/tex]
 
sorry chem_tr is right! (allways right) well, I am sorry for the mix up, my first time posting. thanks for catching that chem!
 
chem_tr said:
The main problem is that you will have to find which reactant is excess, so the other will be the limiting reagent. To find this, you'll use mole calculations. Which one is excess, 10.00 g of O2 or 20 g of NO2? You can use O=16 and N=14 g/mole.
I first learned to do these by looking for how much of B you would need to react with the given amount of A, then decide which of the reactants is in excess then do the calculation through. I later found out that it was a lot easier and faster to just do the entire calculation through for each of the reactants separately then use whichever value gives the lowest yield. Takes a lot less thinking so it's less prone to errors. :smile:
 
Yeah, this is a nice approach indeed. Thank you for reminding this.
 
ok thanks so much for your help guys! until next time =)
 

Similar threads

Rate of reaction and coefficient of the reactan
  • · Replies 6 ·
Replies
6
Views
2K
Elephant toothpaste to fight fires?
  • · Replies 5 ·
Replies
5
Views
4K
Understanding Electrochemistry: Anode and Cathode Reactions
  • · Replies 4 ·
Replies
4
Views
3K
Optimizing Redox Reaction of FeO with H2
  • · Replies 9 ·
Replies
9
Views
7K
Can someone help me out with understanding inorganic chem?
  • · Replies 17 ·
Replies
17
Views
3K
Does anyone know of a thermally-stable endothermic reaction?
  • · Replies 9 ·
Replies
9
Views
3K
Synthesis of Fluorescents AuNCs
  • · Replies 1 ·
Replies
1
Views
2K
Organic reaction mechanism help -- Looking for resources
  • · Replies 10 ·
Replies
10
Views
2K
How Do I Solve Double Displacement Reactions for Chemistry Homework?
  • · Replies 5 ·
Replies
5
Views
3K
Does the Value of K Depend on Initial Reactant and Product Amounts?
  • · Replies 3 ·
Replies
3
Views
2K