Thermodynamics: ATP hydrolysis problem
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- Опубликовано: 8 ноя 2024
- 00:24 Importance of ATP
01:27 ATP hydrolysis
01:56 Assuming ΔG° = -31 kcal / mol
03:01 Relation between equilibrium constant (K) and standard Gibbs free energy (ΔG°)
08:56 Using that in vivo K = 10⁸
11:26 Role of ATP in overcoming Law of Mass Action
Calculation of the equilibrium constant K, assuming that the standard Gibbs energy ΔGº is -31 kcal / mol. Next, the (actual) standard Gibbs energy, accounting for the influence of Mg ⁺², is calculated, using the fact that the actual equilibrium constant K is 10⁸. Finally, the effect of ATP hydrolysis in transforming unfavorable (but necessary) biochemical reactions into thermodynamically favorable ones, is illustrated.
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Sir, thank you so much for explaining this. I wasn't able to get the correct answer for any of the ATP hydrolysis problems as I didn't know about the 10^(-3). You solved my problem. ^.^
(For mobile users)
00:24 Importance of ATP
01:27 ATP hydrolysis
01:56 Assuming ΔG° = -31 kcal / mol
03:01 Relation between equilibrium constant (K) and standard Gibbs free energy (ΔG°)
08:56 Using that in vivo K = 10⁸
11:26 Role of ATP in overcoming Law of Mass Action
Thank you for the video, been working on a problem fro three days. finally finished it. I owe you one. Thanks
I greatly appreciate the breakdown. Very insightful, sir. Thank you.
Glad it was helpful!
Great explanation really😁😁but i gotta ask...why not use 37°C = 310K for normal cell
Good question! I probably should have :(
Thanks for sharing your knowledge! Really enjoyed it. So may I conclude that in the cell of a human body, where the temperature is above 298 K, the standard Gibbs energy is even lower than - 45,65 kJ per mol?
Hello! I am not sure if you are still checking the comments but I have a question on the math.
When you are finding the free Gibbs energy using 10^8 you calculate:
(8.314JK^-1mol * 298K) as -24776Jmol-1 while I am getting 2477.6Jmol-1
Then you state that (-24776Jmol^-1 * 8 * 2.303) equal 45.65kJmol^-1 although I can only seem to get that number w/2477.6 not 24776 (I divide by 1000 to change from J to kJ.
Am I missing a step JK^-1mol becomes Jmol^-1 (multiplying by 1x10^1) or is it a typo?
Thank you for clarifying (biochem is not my forte!)
Yes, it is a typo.
Hey, you are great! Thank you for this
Happy to help!
Thank you 😭😭❤️
Thanks for the video. I have a question regarding the actual physical meaning of negative values of Gibbs energy. Does this mean the products are at a higher kinetic energy (the products move faster)? If so, how is this good for cell synthesis.
The value of the Gibbs energy has several different physical interpretations.
First, the standard Gibbs energy (ΔG°) is the value of ΔG for a reaction aA + bB
↔ cC + dD, when A, B, C, and D each have a concentration of "1" M or atm.
(It is the values of "1" that make it "standard".)
The standard Gibbs energy (ΔG°) is related to the equilibrium constant K, by
ΔG° = -RT ln K.
If ΔG° is positive, then K > 1. If ΔG° is negative, K < 1. If ΔG° = 0, then K = 1.
Second, the sign of ΔG (with no "°") tells us whether the reaction is spontaneous as written. If ΔG is negative, the reaction is spontaneous; if ΔG is positive, the reaction is spontaneous in the opposite direction; and if ΔG = 0, the reaction is at equilibrium. (Very important to know!)
Ultimately, the exact magnitude of the Gibbs energy (ΔG) - more precisely, the Gibbs energy ΔG divided by the thermodynamic temperature T - is related to the change in the entropy S of the universe caused by the reaction. The condition that ΔG be negative for a spontaneous reaction is nothing but the Second Law of Thermodynamics in disguise.
(See here: ruclips.net/video/pKbuLV89QCo/видео.html)
@@lseinjr1 Thanks but that doesn't answer my question. What form is this energy of? Kinetic? Potential? How does ATP hydrolysis produce energy in that reaction? Gibbs is in units of joules so it's energy but which form?
I mentioned the important physical interpretations of the Gibbs energy. ΔG does not have a simple interpretation in terms of kinetic energy.
The enthalpy (ΔH) can be thought of as the change in energy (both potential and kinetic) during a reaction where the pressure remains constant. The energy stored in chemical bonds is an important example of potential energy. It is typically much larger than the kinetic energy. You can do the calculation yourself to confirm.
Biological systems typically operate in a small temperature range. If we assume the temperature is constant, then the average kinetic energy of all molecules is the same. This is a very useful property of the temperature. If the number of molecules changes during a reaction, then there will be a net change in kinetic energy.
The "Gibbs energy" has units of joules per mole. The important quantity is the Gibbs energy divided by temperature, which has units of J / K mol. These are the units of ENTROPY. Ultimately, the Gibbs energy is all about the entropy.
@@lseinjr1 Thanks but I still am not clear. ATP hydrolysis is "an exothermic reaction" which means heat should be released to balance out the loss in enthalpy. In other words, I think the temperature rises and the molecules should move about with higher kinetic energy.
sir its shows 1.251 answer
That is 1.25