A. The change in Gibbs free energy of ATP synthesis (acknowledging the body requires 46.3 kJ/mole) is..
This reaction is endergonic or exergonic?
The energy for ATP synthesis comes from
Is energy used to make ATP transferred in a single reaction or is it the sum of many?
EXPLAIN
C. How much eneegy (precise) could one liberate from one mole of ATP? why?
A. The change in Gibbs free energy of ATP synthesis, acknowledging that the body requires 46.3 kJ/mole, can be determined by the equation ∆G = ∆H - T∆S, where ∆G is the change in Gibbs free energy, ∆H is the change in enthalpy, T is the temperature in Kelvin, and ∆S is the change in entropy. The values of ∆H and ∆S can be obtained experimentally.
B. This reaction is endergonic, meaning that it requires an input of energy to proceed. ATP synthesis is an energy-requiring process.
The energy for ATP synthesis comes from the breakdown of energy-rich molecules, such as glucose, through cellular respiration. The energy released during this process is used to generate ATP.
C. The energy used to make ATP is not transferred in a single reaction but rather is the sum of many reactions. ATP is synthesized in cells through a series of enzymatic reactions called the ATP synthase complex, which involves the transfer of energy from various sources, such as glucose metabolism or light in the case of photosynthesis.
The precise amount of energy that can be liberated from one mole of ATP is approximately 30.5 kJ. This value represents the standard free energy change for the hydrolysis of ATP to ADP and inorganic phosphate (Pi). The release of this energy is due to the breaking of high-energy phosphate bonds in ATP, which releases a considerable amount of energy that can be used for cellular processes.
A. To determine if the reaction of ATP synthesis is endergonic or exergonic, we need to calculate the change in Gibbs free energy (∆G) of the reaction. The Gibbs free energy change (∆G) is calculated using the equation: ∆G = ∆H - T∆S, where ∆H is the change in enthalpy, T is the temperature in Kelvin, and ∆S is the change in entropy.
To find the change in Gibbs free energy of ATP synthesis, we need the values of ∆H and ∆S. If we know that the body requires 46.3 kJ/mole for ATP synthesis, this information likely pertains to ∆H. Assuming standard conditions at 298 K, we can now use the equation to find ∆G. However, we need the value of ∆S as well. If ∆S is not provided, it might require additional information or assumptions to calculate ∆G accurately.
Regarding the source of energy for ATP synthesis, it comes from the catabolic reactions that precede the synthesis. These catabolic reactions, such as cellular respiration or metabolism of nutrients, release energy that can be used for ATP synthesis. In simpler terms, ATP synthesis gets its energy from the breakdown of molecules like glucose during cellular respiration.
Furthermore, the energy used to make ATP is not transferred in a single reaction. It is the sum of many reactions occurring in the body's cells. ATP is synthesized through a process called oxidative phosphorylation in the mitochondria, involving a series of reactions in the electron transport chain.
C. The precise amount of energy that can be liberated from one mole of ATP is approximately 30.5 kJ/mol. This value is in line with experimental observations and calculations. ATP hydrolysis, the breakdown of ATP to ADP and inorganic phosphate (Pi), releases this energy. The released energy can be harnessed by cells to perform various cellular processes, such as muscle contraction, active transport, and chemical synthesis.
The reason why one mole of ATP can liberate this amount of energy can be attributed to the phosphoanhydride bonds present in ATP's structure. These bonds store high-energy phosphate groups, and when hydrolyzed, they release the stored energy. The release of energy occurs due to a change in the chemical bonds, resulting in a more stable state (ADP + Pi). The liberated energy can then be utilized by cellular processes to perform work.