In the turkish dubbing, the guys who write the transkript are so clever. They put good jokes in so that we dont die of boredom. in 2:37 she says that the things we wrote are really helpful but in turkish one the guy says (yes this woman is dubbed by a really good voice actor) "for real im glad i wrote that because its gonna be helpful. No joke for real. not gonna lie." the way he says it is so funny and he laughs as well and i think it is hilarious and really sincere to me. Thanks a lot making me stay in front of my pc to learn more Khan Academy.
If both gases are perfectly mixed, the volume is the same. However, when you increase the pressure of the system, that will increase its temperature, and then you will have an effect over your CO2 partial pressure
What's up with the Khan Academy website using a new video player instead of TH-cam? I cannot modify the playback speed anymore and the subtitle option is not even available. Please revert to TH-cam player on behalf of the community, thank you.
if total pressure increases then using dalton's partial pressure equation the partial pressure of co2 should increases and thus the equilibrium should shift backwards
If it is a closed system and you add Ar(g), wouldn't the volume of the system decrease. causing PCO2 to increase, resulting in the equilibrium shifting to the left? You put more pressure on the system so that everything compresses more, which would be similar to decreasing the volume.
Imagine two scenarios: An infinitesimally small cube of calcium carbonate (CaCO3), and a large chunk of calcium carbonate. Obviously, the large chunk of calcium carbonate will have more surface area. Common sense would have me believe that the increase in surface area means an increase in the forward reaction: CaCO3(s) = CO2(g) + CaO(s). Thus, by adding CaCO3(s), my intuition would be that this favors the forward direction. Le Chateleir's principle tells me this is not the case. "Because the solid is stationary and not dynamic", I understand that part, but still, we are ignoring surface area here. Why?
Stav Shmueli because it’s very hard to consider surface factor ,it is hard to calculate it, in fact if you turn the large solid of CaCO₃ into powder, the forward reaction surly will be faster,but it is difficult to say or calculate how faster it is,so we ignore it.
When you add inert gas like Argon into the reaction it will *increase the volume* and thus it will *decrease the total pressure* but you have said that the total pressure is *increasing* so please clear my *DOUBT*
TECHNICAL SAHITYA 😒😒😒😑😑😑😑😑😑...how its gonna increase the volume of the container??? Volume of the container is gonna remain same..(as its a metal container)...thereby increasing the total pressure!!!
So for Adding CO2 and for increasing the volume the reaction shifts in both cases to the left side? Aren't the reactants also the product? In both cases, the right side needs to react more to establish the equilibrium again? Help!! :(
I know you wrote it 1 year ago, but maybe my comment will help someone else with the same question. Adding CO2 shifts to the right (reactants) because we now have more products added so they will react to create some reactants (CO2+CaO=CaCO3) so they can make equilibrium. They want to come back to the equilibrium that was before we added products so they want to have less products more reactants and to do so they need to react to the left. If we increase volume reaction shifts to the right because we have now a lot of volume with not so much CO2 - low pressure. The reaction wants to go back as it was before so it wants to make pressure higher and while it cannot make volume smaller it can only make more CO2, so the pressure will be higher. That's why reaction goes more to the right side - to create these CO2 (sorry if I made some english mistakes, not my native language)
In the turkish dubbing, the guys who write the transkript are so clever. They put good jokes in so that we dont die of boredom. in 2:37 she says that the things we wrote are really helpful but in turkish one the guy says (yes this woman is dubbed by a really good voice actor) "for real im glad i wrote that because its gonna be helpful. No joke for real. not gonna lie." the way he says it is so funny and he laughs as well and i think it is hilarious and really sincere to me. Thanks a lot making me stay in front of my pc to learn more Khan Academy.
Really nice handwritting
Mhm!
Had to recheck if it's khan coz of the female voice lol
the handwriting is actually so beautiful...
Around the 5:30 mark, you say that there is no shift when you add more of the CaCO3 and im confused why the shift wouldn't be towards the right?
because its a solid and solids do not affect the shift, like adding CaCo would not affect shift.
Your voice is amazing
By adding enough argon it would increase the pressure on CO2 and decrease the volume by concentrating the CO2 into a more confined volume.
If both gases are perfectly mixed, the volume is the same. However, when you increase the pressure of the system, that will increase its temperature, and then you will have an effect over your CO2 partial pressure
What's up with the Khan Academy website using a new video player instead of TH-cam? I cannot modify the playback speed anymore and the subtitle option is not even available. Please revert to TH-cam player on behalf of the community, thank you.
if total pressure increases then using dalton's partial pressure equation the partial pressure of co2 should increases and thus the equilibrium should shift backwards
If it is a closed system and you add Ar(g), wouldn't the volume of the system decrease. causing PCO2 to increase, resulting in the equilibrium shifting to the left? You put more pressure on the system so that everything compresses more, which would be similar to decreasing the volume.
I wanna know that too :(??? It seems like it!
Imagine two scenarios: An infinitesimally small cube of calcium carbonate (CaCO3), and a large chunk of calcium carbonate. Obviously, the large chunk of calcium carbonate will have more surface area. Common sense would have me believe that the increase in surface area means an increase in the forward reaction: CaCO3(s) = CO2(g) + CaO(s).
Thus, by adding CaCO3(s), my intuition would be that this favors the forward direction. Le Chateleir's principle tells me this is not the case. "Because the solid is stationary and not dynamic", I understand that part, but still, we are ignoring surface area here. Why?
Stav Shmueli because it’s very hard to consider surface factor ,it is hard to calculate it, in fact if you turn the large solid of CaCO₃ into powder, the forward reaction surly will be faster,but it is difficult to say or calculate how faster it is,so we ignore it.
Lovely and sweet voice 😄
thanks!
When you add inert gas like Argon into the reaction it will *increase the volume* and thus it will *decrease the total pressure* but you have said that the total pressure is *increasing* so please clear my *DOUBT*
TECHNICAL SAHITYA 😒😒😒😑😑😑😑😑😑...how its gonna increase the volume of the container???
Volume of the container is gonna remain same..(as its a metal container)...thereby increasing the total pressure!!!
This happens only if you add argon at constant pressure
Really cute voice, loved it
So for Adding CO2 and for increasing the volume the reaction shifts in both cases to the left side? Aren't the reactants also the product? In both cases, the right side needs to react more to establish the equilibrium again? Help!! :(
I know you wrote it 1 year ago, but maybe my comment will help someone else with the same question.
Adding CO2 shifts to the right (reactants) because we now have more products added so they will react to create some reactants (CO2+CaO=CaCO3) so they can make equilibrium. They want to come back to the equilibrium that was before we added products so they want to have less products more reactants and to do so they need to react to the left.
If we increase volume reaction shifts to the right because we have now a lot of volume with not so much CO2 - low pressure. The reaction wants to go back as it was before so it wants to make pressure higher and while it cannot make volume smaller it can only make more CO2, so the pressure will be higher. That's why reaction goes more to the right side - to create these CO2
(sorry if I made some english mistakes, not my native language)
Whens your face reveal coming!
Nice, the forward reaction is actually endothermic though but that diagram shows it as exothermic
Yrrr aap pehele hindustan ke logon ko help karo...Uske baad world wide jaao hindi mein bologe toh accha rahe ga
bruh i feel like u look like dillion harper