ICE chart, Equilibrium question

  • Thread starter Thread starter dolpho
  • Start date Start date
  • Tags Tags
    Equilibrium Ice
Click For Summary

Discussion Overview

The discussion revolves around calculating the equilibrium constant (Kc) for the reaction H2(g) + F2(g) <=> 2HF(g) using an ICE chart. Participants are addressing a homework problem that involves determining the correct setup and calculations based on given initial concentrations and equilibrium amounts.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant presents an attempt at setting up the ICE chart and calculating Kc, expressing confusion over the correct answer.
  • Another participant questions the initial concentrations, asking for clarification on whether they are 0.1 or 0.01.
  • A later reply confirms the initial concentrations as 0.01 and 0.05, while seeking further assistance.
  • Multiple participants suggest checking the math, indicating that the derived formula appears correct but the calculated value of Kc is disputed.
  • One participant expresses relief after arriving at the correct answer after a period of stress over the problem.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the correct value of Kc, as there are conflicting calculations and interpretations of the setup. The discussion remains unresolved regarding the final answer.

Contextual Notes

There are indications of potential errors in calculations and assumptions about the initial concentrations, but these remain unverified within the discussion.

dolpho
Messages
66
Reaction score
0

Homework Statement



What is the value of Kc for the reaction H2(g) + F2(g) <=> 2HF(g) given that when 0.010 mol H2 and 0.050 mol F2 are added to a 1.00 L container, 0.0125 mol HF is present at equilibrium.

Homework Equations


The Attempt at a Solution



I'm confused about how to set up the ICE chart in this scenario. We have

H2(g) + F2(g) <=> 2HF(g)

.01... (.05) ... 0
-x ...-x ... 2x
.01-x...(.05-x) ... (.0125)

2x = .0125, x = .00625,

[.0125] ^2 / [.01 - .00625] [ .05-.00625] = 9.3 x 10 ^-6

Which is the incorrect answer, 9.51 ^-1 is right but I'm not sure how to get there. Any help would be appreciated.
 
Last edited:
Physics news on Phys.org
0.1 or 0.01?
 
Borek said:
0.1 or 0.01?

Oops, I'm sorry it's .01, .05, Any ideas :D?
 
Check your math. Formula you derived looks OK to me and its value is not 9.3x10-6. Or at least that's not what I got just by keying it into a calculator.
 
Borek said:
Check your math. Formula you derived looks OK to me and its value is not 9.3x10-6. Or at least that's not what I got just by keying it into a calculator.

Ugh...That feeling when you stress out over a question just to type in the right answer 45 minutes later. Thanks you sir!
 

Similar threads

Chemistry Equilibrium Partial Pressures
  • · Replies 3 ·
Replies
3
Views
3K
What Was the Initial Quantity of Hydrogen Fluoride in the Reaction Jar?
  • · Replies 2 ·
Replies
2
Views
4K
Chemical Equilibrium and Concentration
  • · Replies 5 ·
Replies
5
Views
4K
What Is the Equilibrium Concentration of H2(g) at 1000°C?
  • · Replies 5 ·
Replies
5
Views
4K
Physical Chemistry Homework: Equilibrium Constant and Gas Properties
  • · Replies 5 ·
Replies
5
Views
2K
How Much CO Remains at Equilibrium in a 3L Flask?
  • · Replies 4 ·
Replies
4
Views
5K
What is the Partial Pressure of H2S at Equilibrium?
  • · Replies 19 ·
Replies
19
Views
4K
Calculate equilibrium dissolved oxygen at 19.8 Celsius
  • · Replies 6 ·
Replies
6
Views
3K
Partial pressures and equilibrium question
  • · Replies 3 ·
Replies
3
Views
3K
What are the partial pressures of H2, Br2, and HBr at equilibrium?
  • · Replies 2 ·
Replies
2
Views
10K