To determine: Whether the reaction that has a large negative
Introduction: Exergonic reactions are those reactions for which equilibrium constant is more than 1. Endergonic reactions are those reactions for which the equilibrium constant is less than 1.
To determine: The condition indicated about the equilibrium constant of the reaction.
Introduction: Exergonic reactions are those reactions for which equilibrium constant is more than 1. Endergonic reactions are those reactions for which the equilibrium constant is less than 1.
To determine: Whether the reaction will proceed rapidly to completion if displaced from equilibrium.
Introduction: Exergonic reactions are those reactions for which equilibrium constant is more than 1. Endergonic reactions are those reactions for which the equilibrium constant is less than 1.
To determine: Whether the free energy made available will be more or less.
Introduction: Exergonic reactions are those reactions for which equilibrium constant is more than 1. Endergonic reactions are those reactions for which the equilibrium constant is less than 1.
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Prescott's Microbiology
- For a particular reaction, AH° = −16.1 kJ/mol and AS° = −21.8 J/(mol·K). Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? OT= Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than Karrow_forwardOn the free energy diagram shown, label the intermediate (s) and transition state(s). Is the reaction thermodynamically favorable? Reaction.arrow_forwardA particular reaction has a ΔG‡ of 37.0 kJ mol-1. In the presence of an enzyme, the same reaction has a ΔG‡ of 5.70 kJ mol-1. Calculate the value of ΔΔG‡ in kJ mol-1.arrow_forward
- Consider the analogy of the jiggling box containing coins that was described on page 85. The reaction, the flipping of coins that either face heads up (h) or tails up (T), is described by the equation h ↔ T, where the rate of the forward reaction equals the rate of the reverse reaction.a. What are ΔG and ΔG° in this analogy? b. What corresponds to the temperature at which the reaction proceeds? What corresponds to the activation energy of the reaction? assume you have an “enzyme,” called jigglase, which catalyzes this reaction. What would the effect of jigglase be and what, mechanically, might jigglase do in this analogy?arrow_forwardCalculate the value of AG, if the value of AH is +1200 Kcal/mol, AS is +60 Kcal/mol, and the reaction takes place at 300 K. Once you calculate the value of AG, you can predict the reaction is +16800 Kcal/mol, non-spontaneous/unfavorable - 16800 Kcal/mol, spontaneous/favorable -19200 Kcal/mol, spontaneous/favorable + 19200 Kcal/mol, non-spontaneous/unfavorablearrow_forwardUnder what conditions might a reaction be endothermic but exergonic? Explain.arrow_forward
- Which of the following is TRUE under the following conditions: the enzyme concentration is 2.5 nM, substrate concentration is 75 nM, the KM = 150 nM, and the Vmax = 20 nmol/min a) The rate of the reaction is 20 nmol/min! b) The rate of the reaction is between 10 nmol/min and 20 nmol/min. c) The rate of the reaction is 10 nmol/min. d) The rate of the reaction is below 10 nmol/min. e) The rate cannot be determined from the above information.arrow_forwardConsider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneousarrow_forwardIn the reaction ATP + glucose → ADP + glucose-6-phosphate, ΔG° is -16.7 kJ/mol. Assume that both ATP and ADP have a concentration of 1 M and T = 25°C. What ratio of glucose-6- phosphate to glucose would allow the reverse reaction to occur?arrow_forward
- Can the thermodynamic property Δ G° be used to predict the speed of a reaction in a living organism? Why or why not?arrow_forwardThe equilibrium constant for the reaction Q → R is 25. Solve, (a) If 50 μM of Q is mixed with 50 μM of R, which way will the reaction proceed to generate more Q or more R? (b) Calculate the equilibrium concentrations of Q and R.arrow_forwardWhich of the following statements are true for BOTH the "transition state" and an "intermediate" of reaction? (This is a multi-select question, select all that apply.). Both are only observed in enzyme-catalyzed reactions. Both can be converted to product(s) or might decompose back to the reactant(s). Neither are part of the "net equation" for the reaction. Both contain covalent bonds are in the process of breaking and/or forming. Both are part of every chemical reaction. (i.e. the mechanisms of all chemical reactions, whether enzyme catalyzed or not, will have involve both a transition state and an intermediate).arrow_forward
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