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13. How to calculation standard free energy change of a given biochemical reaction according to its...
13. How to calculation standard free energy change of a given biochemical reaction according to its equilibrium constant, K.? What does it mean for a biochemical reaction when K'>,, or <1? 20. Use an example to explain addition-elimination reactions.
13. How to calculation standard free energy change of a given biochemical reaction according to its equilibrium constant, Kea? What does it mean for a biochemical reaction when Ked'>, -, or <1?
Use standard free energy of formation data to calculate the standard free energy change of reaction, ΔGr0, and the equilibrium constant (molar scale) at 25oC and I = 0 for each of the following reactions: (a) Fe3+ + 6 CN- = Fe(CN)63- (b) Mg2+ + 2 OH- = Mg(OH)20 (c) Mg2+ + 2 OH- = Mg(OH)2(s) (d) Al3+ + F- = AlF2- Some supplementary G0f data (all in kJ/mol): CN-, 172.4; Fe(CN)63-, 729.4, AlF2-, -808.2
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Calculate the equilibrium constant K and the standard free energy change ΔrG˚ at room temperature for the following reaction, HF(aq) H+(aq) + F- (aq) At equilibrium, you measured the following concentrations of reactants and products: [HF]eq = 0.092 M, [H+] eq = 0.008M, [F- ] eq = 0.008 M Think about it: According to your calculation of ΔrG˚, is this reaction reactant favored or product favored? Do you come to the same conclusion when you look at the equilibrium...
1.The spontaneity of system or a biochemical reaction can be determined by: A) Enthalpy alone B) Entropy alone C) Gibbs Free energy D) Temperature and heat 2.A reaction in equilibrium where both forward and reverse reactions are proceeding equally, will have a DELTA G value of: A) Positive B) Zero C) Negative 3.A reaction was originally endergonic, but became exergonic after reducing the temperature. Therefore, this reaction originally had __________ deltaH and a ______ delta S. A) small positive, large...
DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state) for the reaction below is -8.6 kJ/mol. What is ao for this reaction at 37°C when [A)-0.2 M [B-0.2 M, (C]-0.4 M, and ID)-0.6 M? ABCDase A BCD 3.98 J/mol O -4.16 KJ/mol 0-13.22kJ/mol 0 6.81k/moll DI Question 4 2 pts Which one of the following statements is true? 0 if ΔG is negative, the reaction will be spontaneous. Exothermic reactions are always spontaneous....
The standard free energy change for a strong acid-strong base neutralization reaction at 25C° is -79.9KJ. H3O+(aq) + OH-(aq) --> 2 H2O(l) a. Calculate the equilibrium constant for the reaction and explain it's chemical significance.
Below is a free energy change graph for a reaction in which reactants A+B produce the product D. Use the data given to answer the following questions: What does the hump in the middle represent? What is the name of the general class of proteins that are needed to help the reactions go through that hump in a cell? How do they help the reaction go through? In this reaction is the free energy of the reactants or the free...
A reaction has a standard free-energy change of -11.40 kJ mol-1(-2.725 kcal mol-1). Calculate the equilibrium constant for the reaction at 25°C.