A reaction has a ΔG˚′ = -30 kJ/mol, and is considered very favorable. However, the kinetics of this reaction are quite slow Vmax= 25 μmol/min (under saturating conditions, where [S] = 2,000 μM).
Why?
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A reaction has a ΔG˚′ = -30 kJ/mol, and is considered very favorable. However, the kinetics...
5.The following reaction has a ΔG°'--61.9 kJ/mol at 25°C, Phosphoenolpyruvate (PEP) +H2O Pyruvate + Inorganic Phosphate (Pi) (a) Is the reaction favorable under standard biochemical conditions? Explain your answer. (b) What is the equilibrium constant (K) of this reaction at 25°C? In cells the direct hydrolysis of PEP rarely occurs. Rather, the hydrolysis of PEP and the reverse hydrolysis of ATP are coupled (c) w rite out the coupled reaction and determine its ΔG at 25°C The hydrolysis of ATP...
A certain reaction has a ΔG value of 13.8 kJ/mol. What is the value of the equilibrium constant (K) for this reaction when the temperature is 295 K? What is the value of K at 305 K when ∆Go = -4.75 kJ/mol? Consider a process with ∆H = 37.6 kJ and ∆S = 99.5 J/K. At what temperature will this process be at equilibrium?
Consider the hypothetical reaction XY₂(g) --> X(s) + Y₂(g) with ΔG° = +30 kJ/mol XY₂. If you start with 1 atm of XY₂(g), will the reaction occur?
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
A certain reaction has a ΔG value of 13.8 kJ/mol. What is the value of the equilibrium constant (K) for this reaction when the temperature is 295 K?
(10 pts) A chemist is investigating a reaction that has a ΔG。f-5.5 kJ/mol. a) At equilibrium what percentage of the reaction mixture will be products? Show your work. b) Will equilibrium be achieved quickly, slowly, or do you need more information to make that determination? Explain your reasoning
Enolase converts 2-phosphoglycerate (2PG) to phosphoenolpyruvate (PEP). This reaction has a ΔG’o= + 7.5 kJ/mol, but the reaction occurs readily under normal cellular conditions. What is the ratio of [PEP]/[2PG] at equilibrium, at 25oC? In this case, If 2PG is present within the cell cytosol at a concentration of 6 x 10-3M and the concentration of PEP = 0.10 x 10-3M, what is the ΔG of the reaction at 37oC?
. A reaction has the following thermodynamic data: 30 kJ mol-50 J mol K1 a) Compute ΔGo for this reaction at 25 °C. b) Is the reaction spontaneous at 25 C? c) Is the reaction spontaneous at 1000 °C? d) At what temperature does the reverse of this reaction become spontaneous (if in fact there is such a temperature)?
Consider a biochemical reaction under standard conditions. The change in enthalpy is -7 kJ/mol and the change in entropy is -25 JK^-1 mol^-1. Without doing any calculations, can you determine if the reaction is spontaneous? Calculate delta G^degree' for the reaction at 5 degree C. Is the reaction spontaneous or not? Why or why not? If not, does raising the temperature make the reaction more likely to be spontaneous, or less likely to be spontaneous?
1. A reaction has AH = 100 kJ/mol and AS = 250 J/mol K. a. Is the reaction spontaneous at room temperature? b. If not, under what temperature conditions will it become spontaneous? 2. Consider the following reaction at 298 K: N204(g) = 2NO2(g) KP=0.142 What is the standard free energy change at this temperature? Is the reaction spontaneous at this temperature?