I've been here the whole time...where have you been? Glad you finally came across these Breezle and glad they're helpful!

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Thank you.

Glad it was helpful!🙂

Thanks for saying so!

Thanks Qing! Glad you found it helpful!

You're very welcome dude...er I mean Eric!

Excellent, AR - glad the video helped you out!

Awesome Angela and I love it! Congratulations on being in the best profession ever!

You're welcome Alex! Thanks for the feedback

Welcome 😊

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😂😂😂 Yikes!

@@ChadsPrep im not kidding I dropped CHM 2. Now I passed Chem 2!!! Thank you soo much ♥

@@robhousehold You're very welcome and congrats on passing Chem 2! Glad I could be a part of the process!

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Excellent! I do my best to include the common places where errors are made. Glad you found it helpful (but sorry it took 3 hours)!

Glad to hear it - thanks!

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Worth it's weight!

"Hiding" in the vastness of KZfaq - you found me! Thanks for the kind words, kwaku appiah.

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Glad you think so, Brandon - I like your word usage!

You're welcome 😊 - thanks for the comment!

Hey Karl - you mean how it is derived or who derived it?

@@ChadsPrep Thanks for replying! Yes, how or from what basis was it derived?

thanks.

Hi Devika! Delta G standard is simply the delta G value under standard conditions (not at equilibrium). And those standard conditions are where all aqueous reactants and products are present at 1M concentrations and all gaseous reactants and products are present at 1 atm partial pressures. So when delta G standard is negative then we know that the reaction will be spontaneous under standard conditions and will therefore end up at equilibrium having more products than reactants and an equilibrium constant greater than 1 (If delta G standard < 0, then K > 1). And if delta G standard is positive then we know that the reaction will be nonspontaneous under standard conditions (or spontaneous in the reverse direction) and will therefore end up at equilibrium having more reactants than products and an equilibrium constant less than 1 (If delta G standard > 0, then K < 1). Hope this helps!

@@ChadsPrep Hey Chad! Yes I understood that part! But what confuses me is when at equilibrium the new formula becomes delta g standard = -RTlnK so when we solve for this delta g standard does this tell us spontaneity even though we're not at standard conditions? I'm just trying to clarify for myself when to use which formula! Thanks for your help!!

@@devikanair44 So the non-intuituive part of this is that the Equilibrium Constant is mathematically related to the Delta G value under standard conditions. This is not intuitive at all as they correspond to two different conditions: standard conditions and equilibrium. But I think the key is realizing that the equation doesn't imply that they are the same conditions, but just that the Delta G at one condition (standard conditions) is related to the ratio of products to reactants at another condition (Equilibrium). I don't know if this helped untangle it at all for you but I gave it a shot! 🙂

@@ChadsPrep thank you so much, you're amazing!!

Hello Harshit, standard conditions refers to the concentration of aqueous reactants being 1 Molar or gaseous reactants being present with a partial pressure of 1atm, and this is completely independent of any of the coefficients in the balanced reaction. Keep in mind that the coefficients in a balanced reaction NEVER tell you how much of the reactants you have, but simply the ratio in which they react and are produced. Take for example: N2 + 3H2 --> 2NH3 The balance reaction doesn't mean that we have 1 mole of N2 and 3 moles H2. It simply means that N2 and H2 will react in a 1:3 ratio. For every mole of N2 consumed, 3 times as many moles H2 will be consumed at the same time. Hope this helps to clarify!

Happy Studying!

Hello, from U.S.A.

For this to be true you'd be looking for a reaction with an equilibrium constant of 1.0, but you'd also have to manipulate the equilibrium concentrations of the reactants and products to be 1M for it to be considered standard conditions. So while it is possible it would be a somewhat unique reaction under a very unique set of circumstances. Hope this helps!

Chad's Prep It was very helpful. Thank you so much!

A reaction will always proceed to a minimum in free energy which is why for a spontaneous reaction delta G is negative. But once a reaction reaches that minimum point it has reached equilibrium and can go no lower in free energy. So at that point the free energy is no longer changing and delta G is zero. Hope this helps!

@@ChadsPrep Thank you sir

Glad you found the channel!

Happy Studying!

👍 👍

Thanks from U.S.A. - you are counted!

Which part of the video is this about?

Chad's the name - welcome to the channel!