Question

The ΔG° for the hydrolysis of ATP to ADP + Pi is approximately -31 kJ/mol. Calculate the equilibrium constant for this reaction (R = 8.314 J/K/mol) at the cellular temperature of 37°C. If the cellular concentrations of ATP, ADP, and Pi are 8, 1, and 8 mM, respectively, which of the following answers is correct? A. ΔG = 0 B. ΔG = -48.81 kJ/mol C. ΔG = -68.57 kJ/mol D. ΔG = 30.89 kJ/mol

Name: the dg for the hydrolysis of atp to adp pi is approximately 31kjmole calculate the equilibrium constant for this reaction r 8314 jkmole at the cellular temperature of 37c if the cellular con 48231
Uploaded: 2023-07-03T06:32:51-08:00
Duration: 4 min 38 s
Channel: Adi S
Description: the dg for the hydrolysis of atp to adp pi is approximately 31kjmole calculate the equilibrium constant for this reaction r 8314 jkmole at the cellular temperature of 37c if the cellular con 48231

          The ΔG° for the hydrolysis of ATP to ADP + Pi is approximately -31 kJ/mol. Calculate the equilibrium constant for this reaction (R = 8.314 J/K/mol) at the cellular temperature of 37°C. If the cellular concentrations of ATP, ADP, and Pi are 8, 1, and 8 mM, respectively, which of the following answers is correct?
A. ΔG = 0
B. ΔG = -48.81 kJ/mol
C. ΔG = -68.57 kJ/mol
D. ΔG = 30.89 kJ/mol

Added by Martin -.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/03/2023

Step 1

314 J/K/mole, and T = 37°C + 273.15 = 310.15 K. Rearranging the equation to solve for K: K = e^(-ΔG°' / (RT)) K = e^((-31,000 J/mole) / (8.314 J/K/mole * 310.15 K)) K = e^(3.77) K ≈ 43.5 Show more…

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The ΔG° for the hydrolysis of ATP to ADP + Pi is approximately -31 kJ/mol. Calculate the equilibrium constant for this reaction (R = 8.314 J/K/mol) at the cellular temperature of 37°C. If the cellular concentrations of ATP, ADP, and Pi are 8, 1, and 8 mM, respectively, which of the following answers is correct? A. ΔG = 0 B. ΔG = -48.81 kJ/mol C. ΔG = -68.57 kJ/mol D. ΔG = 30.89 kJ/mol