The AG" of hydrolysis (ATP + H2O --> ADP + Pi) is -31.0 kJ/mol. Answer the following questions assuming that the steady-state concentrations in the cell are as indicated below. (Note: Steady-state refers to a non-equilibrium situation that exists due to a balance between reactions that supply and remove these substances.) [ADP] = 0.40 mM, [ATP] = 4.0 mM, and [Pi] = 40.0 mM a) Calculate the equilibrium constant for this reaction. b) What would the AG' for ATP hydrolysis be in the cell? c) Is this reaction at equilibrium in the cell? Briefly explain your answer.
The AG" of hydrolysis (ATP + H2O --> ADP + Pi) is -31.0 kJ/mol. Answer the following questions assuming that the steady-state concentrations in the cell are as indicated below. (Note: Steady-state refers to a non-equilibrium situation that exists due to a balance between reactions that supply and remove these substances.) [ADP] = 0.40 mM, [ATP] = 4.0 mM, and [Pi] = 40.0 mM a) Calculate the equilibrium constant for this reaction. b) What would the AG' for ATP hydrolysis be in the cell? c) Is this reaction at equilibrium in the cell? Briefly explain your answer.
Human Physiology: From Cells to Systems (MindTap Course List)
9th Edition
ISBN:9781285866932
Author:Lauralee Sherwood
Publisher:Lauralee Sherwood
Chapter3: The Plasma Membrane And Membrane Potential
Section: Chapter Questions
Problem 1SQE: Using the Nernst equation, calculate the equilibrium potential for Ca2 and for C1 from the following...
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![The AG" of hydrolysis (ATP + H2O --> ADP + Pi) is -31.0 kJ/mol. Answer the following
questions assuming that the steady-state concentrations in the cell are as indicated below.
(Note: Steady-state refers to a non-equilibrium situation that exists due to a balance
between reactions that supply and remove these substances.)
[ADP] = 0.40 mM, [ATP] = 4.0 mM, and [Pi] = 40.0 mM
a) Calculate the equilibrium constant for this reaction.
b) What would the AG' for ATP hydrolysis be in the cell?
c) Is this reaction at equilibrium in the cell? Briefly explain your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a600697-f443-4c2b-86e3-dc55cb10171e%2F64b71306-942a-423e-a0e5-6c73aaf882a1%2Fd395ugr_processed.png&w=3840&q=75)
Transcribed Image Text:The AG" of hydrolysis (ATP + H2O --> ADP + Pi) is -31.0 kJ/mol. Answer the following
questions assuming that the steady-state concentrations in the cell are as indicated below.
(Note: Steady-state refers to a non-equilibrium situation that exists due to a balance
between reactions that supply and remove these substances.)
[ADP] = 0.40 mM, [ATP] = 4.0 mM, and [Pi] = 40.0 mM
a) Calculate the equilibrium constant for this reaction.
b) What would the AG' for ATP hydrolysis be in the cell?
c) Is this reaction at equilibrium in the cell? Briefly explain your answer.
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