15. Given the following reaction at 298 °K ATP) + H₂O ADP(aq) + P AG= -30.5 kJ R-8.314 J/mol K In a particular cell, the concentrations of ATP, ADP, and P, are 2.7×10 M, 1.1×10 M, and 5.5×10 M, respectively. Calculate the free energy change for the hydrolysis of ATP under these conditions. (Assume a temperature of 298 K)
15. Given the following reaction at 298 °K ATP) + H₂O ADP(aq) + P AG= -30.5 kJ R-8.314 J/mol K In a particular cell, the concentrations of ATP, ADP, and P, are 2.7×10 M, 1.1×10 M, and 5.5×10 M, respectively. Calculate the free energy change for the hydrolysis of ATP under these conditions. (Assume a temperature of 298 K)
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.52QP: Consider the reaction of 1 mol H2(g) at 25C and 1 atm with 1 mol Br2(l) at the same temperature and...
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Transcribed Image Text:15. Given the following reaction at 298 °K
ATP) + H₂O
ADPaq) + Paq) AG= -30.5 kJ
R-8.314 J/mol K
In a particular cell, the concentrations of ATP, ADP, and P, are 2.7×10 M, 1.1×10 M, and 5.5×10 M, respectively.
Calculate the free energy change for the hydrolysis of ATP under these conditions. (Assume a temperature of 298 K)
11. Using the following electrochemical cell, calculate: a) the standard potential, b) the observed potential, and c)
the observed free energy (AG) at 25 °C.
Ce Sa (0.01M), Sn (0.003M) Fe(0.10M), Fe (0.01M) Pt
AE 0.15V (Sn+2e-Sn); AE+0.77V (Fee-Fe) F-96,500 coulombs/mol, T-25 °C
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