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Under cellular conditions ([A] = 8.5 μM, [B] = 1 mM, and T = 37°C, as above), would the left to right reaction (conversion of A to B) be considered endergonic or exergonic? Explain your answer. Consider the following simple chemical reaction that takes place reversibly in the cell under physiological conditions at 37°C. A B AG = -15 kJ/mol for the above (left-to-right) reaction. What is the equilibrium constant (K…) for this reaction under physiological conditions (37°C)? In the cell, which is not at equilibrium, [A] = 8.5 μµM and [B] = 1 mM. What is the free energy change (AG) associated with converting 1 mol of A to 1 mol of B (temperature = 37°C)? at iu

Under cellular conditions ([A] = 8.5 μM, [B] = 1 mM, and T = 37°C, as above), would the left to right reaction (conversion of A to B) be considered endergonic or exergonic? Explain your answer. Consider the following simple chemical reaction that takes place reversibly in the cell under physiological conditions at 37°C. A B AG = -15 kJ/mol for the above (left-to-right) reaction. What is the equilibrium constant (K…) for this reaction under physiological conditions (37°C)? In the cell, which is not at equilibrium, [A] = 8.5 μµM and [B] = 1 mM. What is the free energy change (AG) associated with converting 1 mol of A to 1 mol of B (temperature = 37°C)? at iu

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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Please answer the following: consider the following simple chemical reaction that takes place reversibly in the cell under physiological conditions at 37 celsius. For the first part, delta g is -15 kj/mol. Based on this info, what is the equillibnum constant key for this reaction under physiological conditions (37 celsius)? And the second part asks when it is not at equilibrium, what is the free energy change associated with converting 1 mol of A to 1 mol of B ( temperature=37 celsius)? Final part asks to determine if it's energetic or exergonic? Looking for help particularly for the first and second part with an emphasis on the second part if possible.

Under cellular conditions ([A] = 8.5 μM, [B] = 1 mM, and T = 37°C, as above), would the left to right reaction (conversion of A to B) be considered endergonic or exergonic? Explain your answer.
Transcribed Image Text:Under cellular conditions ([A] = 8.5 μM, [B] = 1 mM, and T = 37°C, as above), would the left to right reaction (conversion of A to B) be considered endergonic or exergonic? Explain your answer.
Consider the following simple chemical reaction that takes place reversibly in the cell under physiological conditions at 37°C. A B AG = -15 kJ/mol for the above (left-to-right) reaction. What is the equilibrium constant (K…) for this reaction under physiological conditions (37°C)? In the cell, which is not at equilibrium, [A] = 8.5 μµM and [B] = 1 mM. What is the free energy change (AG) associated with converting 1 mol of A to 1 mol of B (temperature = 37°C)? at iu
Transcribed Image Text:Consider the following simple chemical reaction that takes place reversibly in the cell under physiological conditions at 37°C. A B AG = -15 kJ/mol for the above (left-to-right) reaction. What is the equilibrium constant (K…) for this reaction under physiological conditions (37°C)? In the cell, which is not at equilibrium, [A] = 8.5 μµM and [B] = 1 mM. What is the free energy change (AG) associated with converting 1 mol of A to 1 mol of B (temperature = 37°C)? at iu
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