How to Calculate Partial Pressures of Gases at Equilibrium?

  • Thread starter Thread starter pmart491
  • Start date Start date
  • Tags Tags
    Partial
Click For Summary

Discussion Overview

The discussion revolves around calculating the partial pressures of gases at equilibrium for the reaction H2 + I2 <-> 2HI, given initial conditions and the equilibrium constant (Keq). Participants explore the application of the ideal gas law and the equilibrium expression in a homework context.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Exploratory
  • Debate/contested

Main Points Raised

  • One participant presents the initial conditions and attempts to calculate the initial pressures of H2 and I2 using the ideal gas law.
  • Another participant emphasizes that changes occur in the system as it reaches equilibrium, suggesting that the pressures of H2 and I2 will not remain the same.
  • There is a discussion about the equilibrium constant (Kp) and its relationship to the partial pressures of the gases involved in the reaction.
  • Participants discuss the changes in moles of H2, I2, and HI, proposing an ICE (Initial, Change, Equilibrium) chart to track these changes.
  • Some participants express uncertainty about the correct representation of the changes in moles and how to set up the equilibrium expression correctly.
  • There is confusion regarding whether to use x or 2x for the change in HI and how to properly incorporate these into the equilibrium expression.
  • Participants clarify that both H2 and I2 decrease by x, while HI increases by 2x, leading to discussions about the correct formulation of the equilibrium expression.
  • There is a suggestion to solve a quadratic equation that arises from the equilibrium expression, with some participants questioning the correct terms to include.

Areas of Agreement / Disagreement

Participants generally agree on the need to calculate changes in moles and pressures to find equilibrium values, but there is disagreement and confusion regarding the correct application of coefficients in the equilibrium expression and the resulting mathematical formulation.

Contextual Notes

Participants express uncertainty about the assumptions made in the calculations, particularly regarding the coefficients in the equilibrium expression and the representation of changes in moles. There are unresolved mathematical steps related to solving the quadratic equation derived from the equilibrium expression.

Who May Find This Useful

Students studying chemical equilibrium, particularly in the context of gas reactions, and those interested in applying the ideal gas law and equilibrium constants in practical scenarios.

pmart491
Messages
19
Reaction score
0

Homework Statement


A 1L flask is filled with 1 mole of H2 and 2 moles of I2 at 448degrees celsius. The value of the Keq for the reaction
H2 + I2 -><- 2HI at 448degrees celsius is 50.5. What are the partial pressures of H2, I2, and HI in the flask at Equilibrium?

All reactants and products are gases. Answer is to be in atm.


Homework Equations


PV=nRT


Pressure of:
H2 I2 HI
I
C
E


The Attempt at a Solution


First, the initial equilibrium of HI is 0 because it doesn't exist yet.
I used PV=nRT to find pressure of H2 and I2
H2) P= 1mole x .0821 x 721K
------------------------- = 59.19atm
1L

I2) P= 2mole x .0821 x 721K
---------------------- = 118.39atm
1L

I need help trying to find what exactly happens after the system reaches equilibrium and how to find the final pressures. Thought: could the pressure of H2 be the same before and after equilibrium because the temperature remains the same? Same for I2?
 
Physics news on Phys.org
I'm way past my bedtime so I'll check much much later but leaving the message here.

H2 + I2 -><- 2HI is an important equation.

You're thinking along the right track, there has to be some changes happening to the system to reach equilibrium.

Thought: could the pressure of H2 be the same before and after equilibrium because the temperature remains the same? Same for I2? No definitely not. I'll explain why down there. Read on.

You see, initially flask has 1 mole of H2, 2 mole of I2 and there is no HI at the start, just because the gases are assumed to be in there first by theory (i.e. not reacted yet). Of course the forward reaction of the equilibrium will happen; Moles of H2 and I2 will decrease and HI will be formed.

By Keq, I kind of found out that it means equilibrium constant, we call it Kp over here.
You should have some kind of equation on the Keq, try look it up, this is my simplified version:

Kp = [Partial Pressure of Reactant(s)]^power of reactant coefficient / [Partial Pressure of Product]^power of product coefficient

Try it out!
 
You've found the initial pressures. Find what the change is for each gas when it goes toward equilibrium, and then find what the equilibrium pressures are. It will consist of a variable.
 
Ok, so I went with Snazzy on this one. for the C in my ICE chart i have the change in Hydrogen as 0 because the moles of hydrogen did not change. I have the change in Iodine, I2, as -x because the number of I2 moles decreased from 2 to 1. Finally I have the change in HI as +2x because it started as 0 moles and increased to 2 moles.

I took this and plugged it in
50.5= Pressure HI
------------------------
Pressure H2 x Pressure of I2

50.5= 2x
-----------------
59.19 x (118.39-x)

50.5= 2x
-----------------
7007.5 - 59.19x
353878.75 - 292989.095x = 2x
353878.75 = 2991.5x

x= 118.29
P H2 I2 HI

I 59.19 118.39 0

C 0 -x +2x

E 59.19 0.10 236.58
 
Last edited:
Hold on, mate. You don't know how many moles exactly will be at equilibrium for each gas. You only know that the change for I2 AND H2 is -x, and the change for HI is +2x.

Using that you can figure out what X is.
 
just so i can understand it, how come H2 is -x AND I2 is -x?
 
Both H2 and I2 start with one mole each. They both have 1 has their coefficient (1H2 + 1I2 -> 2HI).

Both of them will react with each other to produce HI. Thus, an amount of H2 mixes with an equal amount of I2 to produce HI. You don't know how much H2 and I2 react with each other, that's why you leave it as "-X".
 
so,

50.5=
2x
------------------
(59.19-x)(118.39-x) ?

I end up with

50.5=
2x
-----------
x^2 + 177.58x - 7007.5

What am I doing wrong?
 
Last edited:
You're not doing anything wrong. Solve the quadratic that ensues. You're actually missing a squared term for the pressure of HI since the equation gives 2 moles HI for every mole of H2 and I2.
 
  • #10
The question said the flask started out with 1 mole of H2 and 2 moles of I2. So the final should be (1-x) mole of H2 and 2 moles of (2-x) mole of I2 if I'm not wrong. From your steps I think you're doing it fine.

Only that you need to have that [2H]² somewhere as Snazzy says. It's a matter of the power of coefficient, for example if you have α HI instead you will be using [HI]^α...since the equation gives α moles HT for every mole of H2 and I2.
 
  • #11
Snazzy said:
You're not doing anything wrong. Solve the quadratic that ensues. You're actually missing a squared term for the pressure of HI since the equation gives 2 moles HI for every mole of H2 and I2.

oh so its x^2 and not 2x, thanks
 
  • #12
Is it x^2? Or is it (2x)^2?
 
  • #13
HI=x^2 H2=(1-x) and I2=(2-x)...I just have to plug in the numbers now and see what i get.
 
  • #14
Why is it x^2 if the change is 2x for HI?
 
  • #15
this is the ICE chart i have so far

P H2 I2 HI

I 59.19atm 118.39atm 0atm
C (1-x) (2-x) x^2
E 59.19(1-x) 118.39(2-x) x^2

x^2
---------------------------
59.19(1-x) times 118.39(2-x)when i do that i get x=square root of 707757.5 - 1061636.25x + 353878.75x^2
 

Similar threads

Chemistry Equilibrium Partial Pressures
  • · Replies 3 ·
Replies
3
Views
3K
What is the Partial Pressure of H2S at Equilibrium?
  • · Replies 19 ·
Replies
19
Views
4K
Equilibrium and Kp: Find HI Mass at 700K
  • · Replies 1 ·
Replies
1
Views
3K
How to Calculate Total Pressure in a Chemical Equilibrium System?
  • · Replies 1 ·
Replies
1
Views
3K
Final Pressure of Gas Mixture After Reaction Completed
  • · Replies 10 ·
Replies
10
Views
5K
How Do You Calculate Equilibrium Partial Pressures in a Chemical Reaction?
  • · Replies 3 ·
Replies
3
Views
9K
Thermodynamics equilibrium constant problem
  • · Replies 9 ·
Replies
9
Views
3K
How Does Increased Pressure Affect Chemical Equilibrium in the Reaction A⇔2B?
  • · Replies 5 ·
Replies
5
Views
2K
Calculating Final Pressure in a Sublimation and Pressure Homework Problem
  • · Replies 3 ·
Replies
3
Views
6K
Calculate the equilibrium constant Kc for the reaction at this temperature
  • · Replies 6 ·
Replies
6
Views
14K