Did you mean vice versa at 1:38? If it is a mistake please correct it as students might get confused like me. I love your videos and your channel is super helpful!
@@MSJChem "When the Position of equilibrium shifts towards the side with fewer number of gaseous molecules it results in a decrease in pressure", I think it should be, "results in an increase in pressure" Same for the next statement where you say "When the Position of equilibrium shifts towards the side with a greater number of gaseous molecules it results in an increase in pressure", it should be, "results in a decrease in pressure" It's basically the 4 lines at the very bottom of the page which I think are incorrect
Check the wording on the slide - it doesn't say what happens when pressure decreases, it says pressure will decrease when equilibrium moves to the side with fewer molecules, not quite the same thing.
so if the equilibrium shifts to the higher gaseous molecules side then the pressure will increased, , right? But at the same time, you also said if the pressure increased then the equilibrium shifts to the products side (which is having fewer gaseous molecules in your given example)? This was a little bit confusing
The system will try to reverse the changes that you make - so if you increase the pressure, the system will try to decrease the pressure by shifting to the side with fewer gaseous molecules and vice versa.
mister thank you so much I have a question please can you conclude that if mols are equal tso he change of pressure will not affect the the equation ????
@@MSJChem So the K actually should change because of the formula, because the ratio between reactants and products clearly changes, but by agreement it stays constant or what? I asked my chemistry teacher and he couldn't explain. Thanks.
Kc is temperature dependent which means it only changes if the temperature changes. If changes are made to the pressure of the reaction we assume that temperature remains constant so the Kc stays the same.
Did you mean vice versa at 1:38?
If it is a mistake please correct it as students might get confused like me. I love your videos and your channel is super helpful!
@@beanbean54 what did I say?
@@MSJChem
"When the Position of equilibrium shifts towards the side with fewer number of gaseous molecules it results in a decrease in pressure", I think it should be, "results in an increase in pressure"
Same for the next statement where you say "When the Position of equilibrium shifts towards the side with a greater number of gaseous molecules it results in an increase in pressure", it should be, "results in a decrease in pressure"
It's basically the 4 lines at the very bottom of the page which I think are incorrect
Hey Mike,I think you're wrong when pressure is decreased it shifts to the side with more number of moles of the gas and vice versa :)
Which point in the video?
@@MSJChem @1:39 going forward
Check the wording on the slide - it doesn't say what happens when pressure decreases, it says pressure will decrease when equilibrium moves to the side with fewer molecules, not quite the same thing.
thank you! very easy to understand 🥰🥰✨✨
Glad I could help.
Thank you Mike!
I have a question. What if one side has only a solid and a liquid? Does this technically count as 0 moles of gas?
Pressure only effects gaseous reactions.
so if the equilibrium shifts to the higher gaseous molecules side then the pressure will increased, , right? But at the same time, you also said if the pressure increased then the equilibrium shifts to the products side (which is having fewer gaseous molecules in your given example)? This was a little bit confusing
The system will try to reverse the changes that you make - so if you increase the pressure, the system will try to decrease the pressure by shifting to the side with fewer gaseous molecules and vice versa.
can you plz explain me how do we know which side of the reaction has more no. of moles or volume
Add up the coefficients on each side of the equation.
life saver god bless you
Mister,
you are wrong in minute 1:38, it's vice-versa!!
mister thank you so much I have a question please can you conclude that if mols are equal tso he change of pressure will not affect the the equation ????
If there are the same number of gaseous molecules on both sides of the equation then pressure has no effect on the position of equilibrium.
@@MSJChem thank you so much but I need a rule that proves that
What if the reaction has gases and liquids? Is it only the gases that affect then?
For changes in pressure only gases, yes.
What systems are affected by changes in pressure?
In general, gaseous reactions such as the Haber process.
Thank You
Best👍
Wrong ,,,If Pressure increases then reaction shifted to that direction where less no.of mole present
How come Kc doesnt change?
Kc is temperature dependent. It only changes with temperature.
@@MSJChem So the K actually should change because of the formula, because the ratio between reactants and products clearly changes, but by agreement it stays constant or what? I asked my chemistry teacher and he couldn't explain. Thanks.
Kc is temperature dependent which means it only changes if the temperature changes. If changes are made to the pressure of the reaction we assume that temperature remains constant so the Kc stays the same.
You are wrong about the shifting of direction of equilibrium. Just confused the sht outa me for minutes. What a damn waste
May I ask which part of the video you think is wrong?
This guys just confuses the whole concept.
What exactly are you confused about?