**Title: Understanding ATP Hydrolysis and Its Role in Energy Production**A critical reaction in the production of energy necessary to perform work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate (ATP) to adenosine diphosphate (ADP). This reaction is represented by the following equation:\[ \text{ATP(aq)} + \text{H}_2\text{O(l)} \rightarrow \text{ADP(aq)} + \text{HPO}_4^{2-} \text{(aq)} \]In this reaction, the change in free energy (\( \Delta G^\circ_{\text{rxn}} \)) is \(-30.5 \, \text{kJ/mol}\) at a physiological temperature of \(37.0^\circ \text{C}\) and pH of 7.0. **Problem Statement:**Calculate the value of \( \Delta G_{\text{rxn}} \) in a biological cell under the following conditions:- \([\text{ATP}] = 5.0 \, \text{mM}\)- \([\text{ADP}] = 0.30 \, \text{mM}\)- \([\text{HPO}_4^{2-}] = 5.0 \, \text{mM}\)**Input Field:**There is an input field available to enter the calculated value of \( \Delta G_{\text{rxn}} \), expressed in kJ/mol.**Question for Consideration:**Is the hydrolysis of ATP spontaneous under these conditions?- Options: - Yes - NoThis exercise helps students understand the thermodynamics of ATP hydrolysis and its significance in cellular energy transfer.

Answered: Image /qna-images/answer/27a0412c-76ef-4daf-b0de-a26f0686090e.jpg

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H₂O(1)→ ADP(aq) + HPO2 (aq) for which AGxn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGrxn in a biological cell in which [ATP] = 5.0 M, [ADP] = 0.30 mM, and [HPO2¯] = 5.0 mM. AGrxn= Is the hydrolysis of ATP spontaneous under these conditions? yes no kJ/mol

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H₂O(1)→ ADP(aq) + HPO2 (aq) for which AGxn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGrxn in a biological cell in which [ATP] = 5.0 M, [ADP] = 0.30 mM, and [HPO2¯] = 5.0 mM. AGrxn= Is the hydrolysis of ATP spontaneous under these conditions? yes no kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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