If you calculate a value for ∆ G ° for a reaction using the values of Δ G f ∘ in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate ∆ G for a reaction at nonstandard conditions? The equation to determine ∆G at nonstandard conditions has Q in it: What is Q ? A reaction is spontaneous as long as ∆ G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why don’t reactions move away from equilibrium?
If you calculate a value for ∆ G ° for a reaction using the values of Δ G f ∘ in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate ∆ G for a reaction at nonstandard conditions? The equation to determine ∆G at nonstandard conditions has Q in it: What is Q ? A reaction is spontaneous as long as ∆ G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why don’t reactions move away from equilibrium?
Solution Summary: The author explains that thermodynamics is associated with heat, temperature, and its relation with energy and work. It helps predict whether a process will take place or not.
If you calculate a value for ∆G° for a reaction using the values of
Δ
G
f
∘
in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate ∆G for a reaction at nonstandard conditions? The equation to determine ∆G at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as ∆G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why don’t reactions move away from equilibrium?
Please answer the question and provide a detailed drawing of the structure. If there will not be a new C – C bond, then the box under the drawing area will be checked.
Will the following reaction make a molecule with a new C – C bond as its major product:
Draw the major organic product or products, if the reaction will work. Be sure you use wedge and dash bonds if necessary, for example to distinguish between major products with different stereochemistry.
Please do not use AI. AI cannot "see" the molecules properly, and it therefore gives the wrong answer while giving incorrect descriptions of the visual images we're looking at. All of these compounds would be produced (I think). In my book, I don't see any rules about yield in this case, like explaining that one product would be present in less yield for this reason or that reason. Please explain why some of these produce less yield than others.
Biochemistry: Concepts and Connections (2nd Edition)
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The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY