Please do not stop doing the good job you are doing, its unfortunate the education system is so poor that we have to go to TH-cam for help from brilliant minds like yourself. Thanks again, Some of these college professors need training on how to teach I swear.
Wow, I knew that spontaneous processes could be slow, but the diamond to graphite example still amazed me. Gives me a whole new appreciation for the difference between thermodynamically-favored verses kinetically favored.
At 3:45 of the video you mentioned that after the gas expands the temperature of the gas wouldn't change. However, I believe the temperature of the gas would indeed decrease rather than remaining same.
So basically, spontaneity only has to do with whether the products or reactants are favored? Just having some trouble wrapping my head around this concept.
Great video, quick question when you say spontaneous required no external energy source, dont all reactions need activation energy to start them off? Little confused with the two concepts? Thanks again for the informative content.
Zahra think about activation energy as an energy to initiate a reaction. for example, “ combustion “ if there is a gas ( flammable ) spread out into vacuum, no reaction will occur with the oxygen until you initiate it with a spark or a match so it can break the bonds and reaction occurs. once you initiate it you do nothing to can make it continue ( spontaneous ) it is self-sustaining .so all of this is after energy supplied from an external source “ the spark “
How are products favored in a spontaneous reaction? I thought if delta H was negative, it would be exothermic and so move in the backwards direction, reactants favored.
+Renzo Andre What you're referring to is an equilibrium reaction. When the enthalpy change of the reaction is exothermic, then the backward reaction is favored. That's not what he is talking about. He is talking about the spontaneity of a reaction. For example matchstick head burning will cause heat energy to be given out and therefore be exothermic in nature. The burning head also turns to gas and this increases disorder of the system and therefore, entropy. The matchstick burning is not an equilibrium reaction. Energy tends to move towards a lower state so, when you burn the match the products will have lesser energy right? So, the reaction favors product formation. This shows that enthalpy decreases. Hope that helped!
a. Liquid water freezing at a temperature below its freezing point b. Liquid water freezing at a temperature above its freezing point c. The combustion of gasoline d. A ball thrown into the air e. A raindrop falling to the ground f. Iron rusting in a moist atmosphere spontaneous or non spontaneous
My old college chemistry text says that when delta G is equal to "0", then the reaction is at equilibrium just as you do, however, when delta G is "0" and K=1, the products and reactants are equal in concentration but the reaction is not necessarily at equilibrium. My old text goes on to define equilibrium to be when the forward and reverse "reaction rates" are equal. When this condition is met, the reaction can be shifted to the right or to the left depending on the reaction and the value of K. In other words K defines if the reaction lies to the right or to the left or in the middle when the reaction is at equilibrium. So I am confused as to why you and my text say that when delta G is equal to "0", the reaction is at equilibrium?
By the way, as an example. Graphite DOES transform into Diamond spontaneously, but only at very specific conditions ( 1500 K, aprox 60.000 atm pressure) Spontaneity is defined with thermodynamic conditions imposed, such as Temperature and Pressure. Graphite DOES NOT transform into Diamond at 298 K and 1 atm pressure, under these condition the opposite process is spontaneous. As an added note, Enthalpy and Entropy of reaction have nothing to do with reaction rate, the reason at 298K and 1 atm diamonds don't just burst into graphite (exothermic process by the way) , is because this process is kinetically limited by a huge activation energy, which does NOT depend on thermodynamics.
Please do not stop doing the good job you are doing, its unfortunate the education system is so poor that we have to go to TH-cam for help from brilliant minds like yourself.
Thanks again,
Some of these college professors need training on how to teach I swear.
Wow, I knew that spontaneous processes could be slow, but the diamond to graphite example still amazed me. Gives me a whole new appreciation for the difference between thermodynamically-favored verses kinetically favored.
thank you so much for using the simulation. it made it so easy to grasp the concept
th-cam.com/users/shortsDRtHEDvr1wI
Hi. When we're taught about this here in England, we often use the word 'feasible' instead of 'spontaneous'.
You have no idea how helpful this clarification was. Thank you for pointing this out.
Feasible? Wow
thank you
Spontaneous processes can still occur if enthalpy change is positive, as long as T*delta S is much much larger.
th-cam.com/users/shortsDRtHEDvr1wI
At 3:45 of the video you mentioned that after the gas expands the temperature of the gas wouldn't change. However, I believe the temperature of the gas would indeed decrease rather than remaining same.
Thank you so much for the video, every time I'm stuck with chemistry concepts, I always go to your channel.
th-cam.com/users/shortsDRtHEDvr1wI
Has anyone else just binge watched these videos? Love watching them...they are very informative!
i love you bozeman!
THANX , a lot of information , gtta watch it again .
This has been very helpful. Thank you.
Thank you for doing this video. It helps a lot!
So basically, spontaneity only has to do with whether the products or reactants are favored? Just having some trouble wrapping my head around this concept.
Excellent! I hope you post a new videos!!!
th-cam.com/users/shortsDRtHEDvr1wI
Great video, quick question when you say spontaneous required no external energy source, dont all reactions need activation energy to start them off? Little confused with the two concepts?
Thanks again for the informative content.
Zahra think about activation energy as an energy to initiate a reaction. for example, “ combustion “ if there is a gas ( flammable ) spread out into vacuum, no reaction will occur with the oxygen until you initiate it with a spark or a match so it can break the bonds and reaction occurs. once you initiate it you do nothing to can make it continue ( spontaneous ) it is self-sustaining .so all of this is after energy supplied from an external source “ the spark “
thank you that was so helpful
How are products favored in a spontaneous reaction? I thought if delta H was negative, it would be exothermic and so move in the backwards direction, reactants favored.
+Renzo Andre What you're referring to is an equilibrium reaction. When the enthalpy change of the reaction is exothermic, then the backward reaction is favored. That's not what he is talking about.
He is talking about the spontaneity of a reaction. For example matchstick head burning will cause heat energy to be given out and therefore be exothermic in nature. The burning head also turns to gas and this increases disorder of the system and therefore, entropy. The matchstick burning is not an equilibrium reaction.
Energy tends to move towards a lower state so, when you burn the match the products will have lesser energy right? So, the reaction favors product formation. This shows that enthalpy decreases.
Hope that helped!
a. Liquid water freezing at a temperature below its freezing point
b. Liquid water freezing at a temperature above its freezing point
c. The combustion of gasoline
d. A ball thrown into the air
e. A raindrop falling to the ground
f. Iron rusting in a moist atmosphere
spontaneous or non spontaneous
informative!
Spot. On.
Thank you so much
Hello, Mr Anderson. 😎
What do you mean when you say the products are favoured?
It means the reaction makes more products than reactants
Okay, thank you!
When we make both chambers in contact and gas move to right why there is no change in temp and what happens to internal energy.Please explain
Very digestible, thank you for the video!
th-cam.com/users/shortsDRtHEDvr1wI
thank you sir nice method your teaching
When he says occur I hear okurr
nice video
Earned my subscription :)
how can a reaction be reversible if it is favorable one way and unfavorable the other?
Both reactions occur at the same time but, one goes more to completion than the other
Thanks, & nice presentation
book mark 01:14
Thx
But, but, but, but ... diamonds are forever :(
"tending to infinity relative to an average human life span", so if your lover happens to say something like that, now you know what to say
My old college chemistry text says that when delta G is equal to "0", then the reaction is at equilibrium just as you do, however, when delta G is "0" and K=1, the products and reactants are equal in concentration but the reaction is not necessarily at equilibrium. My old text goes on to define equilibrium to be when the forward and reverse "reaction rates" are equal. When this condition is met, the reaction can be shifted to the right or to the left depending on the reaction and the value of K. In other words K defines if the reaction lies to the right or to the left or in the middle when the reaction is at equilibrium. So I am confused as to why you and my text say that when delta G is equal to "0", the reaction is at equilibrium?
nice explaination
Nice one
great explaination. please reduce the pace a lil bit. thanx
I knew id return from HS
useful...
By the way, as an example.
Graphite DOES transform into Diamond spontaneously, but only at very specific conditions ( 1500 K, aprox 60.000 atm pressure)
Spontaneity is defined with thermodynamic conditions imposed, such as Temperature and Pressure.
Graphite DOES NOT transform into Diamond at 298 K and 1 atm pressure, under these condition the opposite process is spontaneous.
As an added note, Enthalpy and Entropy of reaction have nothing to do with reaction rate, the reason at 298K and 1 atm diamonds don't just burst into graphite (exothermic process by the way) , is because this process is kinetically limited by a huge activation energy, which does NOT depend on thermodynamics.
can you talk any faster?