Why doesn't addition of inert gas at constant volume shift the rxn towards one direction
When adding an inert gas in a closed vessel , the total volume is constant so the total pressure has to increase.
But change in total pressure should shift the rxn towards one end (if delta Ng isnt zero)
But that doesnt happen. Please help me understand why this is the case
19 Replies
@Dexter
Note for OP
+solved @user1 @user2... to close the thread when your doubt is solved. Mention the users who helped you solve the doubt. This will be added to their stats.pcl5 converts to pcl3 and cl2
ismei ne dala toh kuch bhi react nahi karega, thus the eqbm conc remains same and reactions quotient too. so theres no change in eqbm
go to the basics. why would a change be warranted? if partial pressure changes then that could cause an overall change
when total volume is constant, adding gases increases the total pressure, but
partial pressure = does that change or not? think about it
i have done the math in my videos, you can do so too just take initial moles to be 1 : 1 and add another mol of gas (hypothetical case)
key being: partial pressure of the individual reactants matters, not the total pressure :)
but I thought that partial pressure of a component was related to the mole fraction of that component.
so a decrease in mole fraction should change it
Yea a diffrence in mile fraction would change it na... But moles aren't changing only the total pressure is changing am I right? I can't open the voice not from sir idk what's wrong
When youre adding a gas obviously the total moles in that closed system would increase
And since volume cant increase the total pressure in the system would increase as well
Oh yea sorry I was high on equilibrium to realise that sori bru
Iski kuch to reasoning humare sir ne samjhayi thi ab yaad ni aa rahi ;-;
revisit the definitions...partial pressure is defined as the pressure of a particular gas exerted on the walls of container when it alone occupies the container
so if i am right, at const vol, there is no change in partial pressure due to no change in vol and no reaction of inert gas with the gas present in container
Shall we close this out? @Neko
yeah but partial pressure is also defined as the molar percent of a gas multiplied by total pressure
Sir suppose there A+B forming C
There are 1-x moles of A and B and x of C
mole percent of A and B is 1-x/2-x and C is x/2-x
Hence partial pressures are (1-x)(P)/(2-x) and (x)(P)/(2-x)
Kp=(x)/(1-x)^2(2-x)(P)
Now if we add 2x moles of an inert gas E, total moles are 2+x
New mole percents are 1-x/2+x and x/2+x
new partial pressures are (1-x)P/2+x and (x)(P)/2+x
Qp=(x)/(1-x)^2(P)(2+x)
Qp is only equal to Kp in this scenario when delta Ng=0
So its still wrong 😢 unless the thing slembash said was true
Or maybe that the change in total pressure cancels out this change in mole fraction
But for that total pressure should decrease after adding inert gas which is obviously wrong
The more I think the more questions I get and I am just getting more confused 💀
Aur yaha kal is cheez ka test hai aur ye hum bhul gaye
we good?
this topic was too confusing for me tbh so yeah you can close it
Are! Video dekha?
+fsolved
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