Question

If the synthesis of ATP from ADP and Pi is +30.5 kJ/mol, what is the minimum...

If the synthesis of ATP from ADP and Pi is +30.5 kJ/mol, what is the minimum amount of energy needed from a reaction to drive ATP synthesis??

Science   Biology   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Synthesis of ATP from ADP and Pi requires +30.5kJ/mol energy. This is a non-spontaneous, endothermic reaction and hence must be coupled to an exothermic, spontaneous process with free energy at least equal to that required to synthesized ATP or more than that. Hence, the minimum energy required to drive ATP synthesis from ADP and Pi of concentration 1M is 30.5kJ/mol. However, because the actual physiological concentrations of ATP, ADP, and Pi are not 1 M, the free energy required to synthesize ATP under physiological conditions is different from that of standard condition.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The energy released is -151 kJ/mol. This energy can be converted into the synthesis of ATP...
The energy released is -151 kJ/mol. This energy can be converted into the synthesis of ATP at an efficiency of 0.7 (70% of the energy released is captured in ATP synthesis) and the oxidation of 1 succinate leads to the phosphorylation of 2 equivalents of ATP. Under these conditions, what is the maximum ratio of [ATP]/[ADP] attainable by oxidative phosphorylation when [Pi] = 1 mM? (Assume the free energy needed for ATP synthesis is +30.5 kJ/mol)
The standard free energy change for ATP hydrolysis is -30.5 kJ/mol. Therefore, the free energy change...
The standard free energy change for ATP hydrolysis is -30.5 kJ/mol. Therefore, the free energy change for this reaction in a cell in which the concentration of ATP, ADP, and Pi are 3.1 mM, 2.2 mM and 6.8 mM, respectively, and assuming a physiologically relevant temperature (37 °C), is: Answer -44.25 kJ/mol explain
The standard Gibbs free energy change for hydrolysis or pure ATP to pure ADP is -31KJ/mol....
The standard Gibbs free energy change for hydrolysis or pure ATP to pure ADP is -31KJ/mol. The reaction is written ATP = ADP +Pi. What is the Gibbs energy of reaction in an environment at 37 C in which the ATP, ADP, and Pi concentrations are all 1mmol/L or 1 µmol/L?
How many ATP equivalents (ATP -> ADP + Pi) are needed to make a 200 amino...
How many ATP equivalents (ATP -> ADP + Pi) are needed to make a 200 amino acid polypeptide from a mRNA template, amino acids and tRNA molecules. GTP -> GDP + Pi counts as one ATP equivalent and ATP -> AMP + 2 Pi counts as 2 equivalents.
The glycolytic reaction glyceraldehyde 3-phosphate + Pi → 1,3-bisposphoglycerate has a ΔG°′ of +6.3 kJ/mol. In...
The glycolytic reaction glyceraldehyde 3-phosphate + Pi → 1,3-bisposphoglycerate has a ΔG°′ of +6.3 kJ/mol. In cells however, it is coupled to the subsequent reaction: 1,3- bisposphoglycerate + ADP → ATP + 3-phosphoglycerate which for which G°’= –18.5 kJ/mol Calculate the free energy change for these two reactions if they are coupled together. This was also given if helpful: Abbreviations for cofactors such as NADH, ATP etc. are sufficient unless the specific structure for that molecule is requested. Otherwise use...
The most recent estimates for the stoichiometry of ATP synthesis from the oxidation of NADH are...
The most recent estimates for the stoichiometry of ATP synthesis from the oxidation of NADH are 2.5 ATP/NADH. Given that the standard-state free energy change in oxidizing NADH with oxygen is -220 kJ/mol (-52.6 kcal/mol), then what is the efficiency, expressed as a percent to the nearest ones, of ATP synthesis in cells if the cost of ATP synthesis is 11.7 kcal/mol?
The direct phosphorylation of glucose by inorganic phosphate is a thermodynamically unfavorable reaction: glucose+Pi→glucoseglucose+Pi→glucose-66-phosphate+H2Ophosphate+H2O ΔG∘′=+3.3kcal/molΔG∘′=+3.3kcal/mol In...
The direct phosphorylation of glucose by inorganic phosphate is a thermodynamically unfavorable reaction: glucose+Pi→glucoseglucose+Pi→glucose-66-phosphate+H2Ophosphate+H2O ΔG∘′=+3.3kcal/molΔG∘′=+3.3kcal/mol In the cell, glucose phosphorylation is accomplished by coupling the reaction to the hydrolysis of ATPATP, a highly exergonic reaction: ATP+H2O→ADP+PiATP+H2O→ADP+Pi ΔG∘′=−7.3kcal/molΔG∘′=−7.3kcal/mol Typical concentrations of these intermediates in yeast cells are as follows: [glucose-6-phospate] = 0.08mMmM [ATP]=1.8mM[ATP]=1.8mM [Pi]=1.0mM[Pi]=1.0mM [ADP]=0.15mM[ADP]=0.15mM Assume a temperature of 25∘C∘C for all calculations. What minimum concentration of glucose would have to be maintained in a yeast cell for the coupled reaction...
For the hydrolysis of ATP to ADP + ℗i, the free-energy change is -7.3 kcal/mol under...
For the hydrolysis of ATP to ADP + ℗i, the free-energy change is -7.3 kcal/mol under standard conditions (1 M concentration of both reactants and products). In the cellular environment, however, the free-energy change is about -13 kcal/mol. What can we conclude about the free-energy change for the formation of ATP from ADP and ℗i under cellular conditions?
Now for some calculations. ATP formation is a nonspontaneous process. It requires energy input. Under standard...
Now for some calculations. ATP formation is a nonspontaneous process. It requires energy input. Under standard state conditions the delta Go’ is ~30 kJ/mol. If the best available measures in a particular tissue indicate cellular levels of ATP= 2.5 mM, ADP = 0.6 mM and Pi =0.2 mM, what value will you report as the delta G naught’ for ATP synthesis? Show all work
The ΔG’o for the hydrolysis of phosphoarginine to arginine and Pi is – 32 kJ/mol. What...
The ΔG’o for the hydrolysis of phosphoarginine to arginine and Pi is – 32 kJ/mol. What is the actual free-energy change (ΔG) for the reaction at 25oC and pH 7.0 in resting lobster muscle where the concentrations of phosphoarginine, arginine, and Pi are: 6.8 mM, 2.6 mM, and 5 mM respectively.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT