The standard free energy of the hydrolysis of ATP to ADP: ATP (aq) → ADP (aq) + (aq) phosphate in solution is ∆G^0 = -313kJ/mol at 37˚C, 1 atm, all solutes are in their standard states at 1 mol/L Assume ideal solution behaviour. a) For a ratio of ATP to ADP of 10, what must be the concentration of phosphate to obtain ∆G = -40.0 kJ/mol for the hydrolysis? b) If the ratio of ATP to ADP is 10, what is the concentration of phosphate at equilibrium? What do you
The standard free energy of the hydrolysis of ATP to ADP: ATP (aq) → ADP (aq) + (aq) phosphate in solution is ∆G^0 = -313kJ/mol at 37˚C, 1 atm, all solutes are in their standard states at 1 mol/L Assume ideal solution behaviour. a) For a ratio of ATP to ADP of 10, what must be the concentration of phosphate to obtain ∆G = -40.0 kJ/mol for the hydrolysis? b) If the ratio of ATP to ADP is 10, what is the concentration of phosphate at equilibrium? What do you
Chemistry by OpenStax (2015-05-04)
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Chapter16: Thermodynamics
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The standard free energy of the hydrolysis of ATP to ADP: ATP (aq) → ADP (aq) + (aq) phosphate in solution is ∆G^0 = -313kJ/mol at 37˚C, 1 atm, all solutes are in their standard states at 1 mol/L Assume ideal solution behaviour.
a) For a ratio of ATP to ADP of 10, what must be the concentration of phosphate to obtain ∆G = -40.0 kJ/mol for the hydrolysis?
b) If the ratio of ATP to ADP is 10, what is the concentration of phosphate at equilibrium? What do you
conclude from your answer (i.e., is the hydrolysis practical based on phosphate concentration)?
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