Consider the following chemical reaction: Glucose + ATP → Glucose-6-Phosphate + ADP + Pi Given the following information, calculate the actual free energy change (G’) of this reaction. G’ of Glucose + ATP → Glucose-6-Phosphate + ADP + Pi = -16.7 kJ/mol [Glucose] = 5.0 mM [ATP] = 1.85 mM [Glucose-6-Phosphate] = 0.083 mM [ADP] = 0.14 mM [Pi] = 1.0 mM Temperature = 37 C R (Gas Constant) = 8.314 J/mol•K

Intramitochondrial ATP concentrations are about 5 mM, and phosphate concentration is about 10 mM. Consider that ADP is five times more abundant than AMP.   a. Calculate the molar concentrations of ADP and AMP at an energy charge of 0.85.   b. Calculate ∆G' for ATP hydrolysis under these conditions (∆G0' for ATP hydrolysis is -32.2 kJ/mol)       The energy charge is defined as ( [ATP] + 1/2 [ADP] ) / ( [ATP] + [ADP] + [AMP] )

The Nutrition Facts label on most food products shows % daily values based on a food energy requirement of 8,360 kJ (2,000 kcal) at normal resting state. a) Assuming that the efficiency of converting food energy to ATP is 50%, calculate the mass of ATP (in kg) that is harvested daily by the human body from 8,360 kJ of food energy. A total of 30.5 kJ of energy is needed to synthesize one mole of ATP under standard conditions. The molar mass of ATP is 505 g/mol. b) For an average 68-kg (150 lbs.) human adult, calculate the % mass of extracted ATP (from your answer in 2a) relative to body weight.

Only 15-14