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![A 70 kg (154 lb) adult requires a calorie intake of 2,000 kcal (8,360 kJ) of food per day
(24 h). The food is metabolized and the free energy is used to synthesize ATP
for useful work. [FYI: Each calorie ("Calorie") listed on food labels corresponds to
1.0 kcal in biochemical terms; the formula weight of ATP is 505 g/mol; and eh mole of
ATP is equivalent to 30.5 kJ]. Assuming that the efficiency of converting food energy
into ATP is 50%, calculate the following:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5ef5f725-b08b-4f71-a80c-f37e47d07785%2Fd3f8fd5c-c0d9-414a-887c-49c3e93e92c6%2Fox0a3om_processed.jpeg&w=3840&q=75)
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- The hydrolysis of the phosphoester bond of ATP releases a large amount of free energy. True or false?if an 8.4-oz (250 mL) energy drink can has 27 grams of sugar, calculate the moles of ATP produced in the body when 1 oz of the drink is consumed assuming all the sugars in 1 oz of the drink are composed of only glucose.How many ATP molecules could maximally be generated from one molecule of glucose, if the complete oxidation of 1 mole of glucose to CO2 and H2O yields 686 kcal of free energy and the useful chemical energy available in the high- energy phosphate bond of 1 mole of ATP is 12 kcal?
- The hydrolysis of ATP to yield AMP and PPi yields_____________ kJ/molWhich of the following compounds would you expect to liberate the least free energy when hydrolyzed? Explain. a. ATP b. ADP c. AMP d. phosphoenolpyruvate e. phosphocreatineConsider 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
- The cleavage of ATP’s phosphoanhydride bond to form ADP yields approximately _____________ kJ/mol..Would you expect an increase or a decrease of entropy to accompany the hydrolysis of phosphatidylcholine to the constituent parts (glycerol, two fatty acids, phosphoric acid, and choline)? Why?Given that the standard free-energy change for the reaction glucose + Pi →glucose 6-phosphate is 13.8 kJ/mol, and the standard free-energy change forthe reaction ATP → ADP + Pi is −30.5 kJ/mol, what is the free-energychange for the reaction glucose + ATP → glucose 6-phosphate + ADP?
- A camel hump contains 12 kg of triacylgylcerols. (a) Given that there are 0.491 moles of ATP per gram of fat, how many moles of ATP could be produced by the fat in the camel hump?(b) If the hydrolysis of ATP releases 7.3 kcal/mole, how many kilocalories are produced by the utilization of the fat?A total of 30.5 kJ mol-1 of free energy is needed to synthesise ATP from ADP and Pi when the reactants and products are at 1.0 M concentrations and the temperature is 25oC. Because the actual physiological concentrations of ATP, ADP, and Pi are not 1.0 M, and the temperature is 37oC, the free energy required to synthesise ATP under physiological conditions is actually ~ 46.2 kJ mol-1. A 68 kg adult requires an energy intake of 8,550 kJ of food per day (24 hours). Calculate the mass (in Kg) of ATP synthesised by a human adult in 24 hours, assuming that the percentage efficiency of converting inputted calories in ATP is 50%. What percentage of the body weight does this represent?If the DGo for ATP hydrolysis into ADP + inorganic phosphate is -7.3 kcal/mole, and the DGo for sucrose synthesis from glucose + fructose is +5.5 kcal/mole, calculate standard free energy change for the combined reaction of ATP + glucose + fructose g ADP + sucrose + inorganic phosphate. DGo = -12.8 kcal/mole DGo = -1.8 kcal/mole DGo = 0 kcal/mole DGo = +1.8 kcal/mole DGo = +12.8 kcal/mole