Question

Suppose the reaction A + B --> C + D has a Δ G of +...

Suppose the reaction A + B --> C + D has a Δ G of + 5.2 kcal/mol. If this reaction is coupled to the reaction ATP + H2O --> ADP + Pi, which has a Δ G of -7.3 kcal/mol. What will be the change in free energy of the combined reaction, and will the reaction be spontaneous? Explain your answer.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A    +    B ------------------------> C   +    D ΔG =   + 5.2 kcal/mol.

ATP   +   H2O -----------------------> ADP + Pi ΔG =   -7.3 kcal/mol

------------------------------------------------------------------------------------------------------------

A + B + ATP + H2O --------------> C + D+ ADP + Pi       ΔG =   - 2.1 kcal/mol

ΔG =   -2.1 kcal/mol . is negative. so reaction is spontenous.

if delta G is positive then the reaction is non-spontaneous.

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
2. Consider the biosynthetic reaction between glutamate and NH4+ to form glutamine at T = 25o...
2. Consider the biosynthetic reaction between glutamate and NH4+ to form glutamine at T = 25o C (R = 8.3145 J / mol∙K), glutamate + NH4+ --> glutamine 2a. The equilibrium constant for the reaction under standard biochemical conditions is Keq = 0.00325. Calculate ΔGo' and please give your answer in kcal/mol (assume RT = 0.6 kcal/mol). ΔGo' = __________ kcal/mol 2b. To make the reaction spontaneous, what would the concentration of glutamine have to be maintained at relative to...
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...
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...
If it costs 10.5 kcal/mol to “run” a particular cation ATPase “pump”, then what is the...
If it costs 10.5 kcal/mol to “run” a particular cation ATPase “pump”, then what is the minimum concentration of ATP required to provide just enough energy to run this ATPase? In other words, what does the concentration of ATP need to be so that the free energy of ATP hydrolysis is -10.5 kcal/mol. Report your answer to the nearest tenth of a mM, and assume that [\Delta] ΔG°' is -7.3 kcal/mol, the concentration of Pi is 3.4 mM, the concentration...
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?
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
If the intracellular concentrations of a metabolite (M-COO-) and its phosphorylated form (M-COOPO32-) were 3 mM...
If the intracellular concentrations of a metabolite (M-COO-) and its phosphorylated form (M-COOPO32-) were 3 mM and 0.12 mM, respectively, and if the intracellular concentrations of ATP and ADP were 3.9 mM and 0.14 mM, respectively, what would be the numerical value of \Delta Δ G (in kcal per mol to the nearest hundredth) for the following reaction: M-COO- + ATP <--> M-COOPO32- + ADP? Assume a temperature of 37 °C and a pH of 7.2. To solve this problem,...
*True or False: Long, weak bonds (like those found in non-polar C-H bonds) have higher potential...
*True or False: Long, weak bonds (like those found in non-polar C-H bonds) have higher potential energy than short, strong bonds (like those found in polar O-H bonds). Adenosine triphosphate (ATP) can be hydrolyzed to become ADP and inorganic phosphate. It has a deltaG of -7.3 kcal/mol. This reaction… (Choose ALL correct answers) [] is exergonic. [] is endothermic. [] releases energy. [] is spontaneous. Changes in free energy are related to both enthalpy and entropy. Which equation best represents...
3. Two amino acids can join together via a peptide bond to make a dipeptide. Below...
3. Two amino acids can join together via a peptide bond to make a dipeptide. Below is an example of such a reaction. glutamate + cysteine  γ-glutamylcysteine ΔG°’ at 25°C for this reaction is 10 KJ/mol; assume 25°C in answering the following. a. Does the ΔG°’ indicate that formation of γ-glutamylcysteine is favored? Explain your answer; no calculations required. b. What is Keq’ for this reaction? c. In certain conditions, the formation of γ-glutamylcysteine can be coupled to ATP...
A: Phosphocreatine is used by your muscle cells to store energy. The dephosphorylation of phosphocreatine, like...
A: Phosphocreatine is used by your muscle cells to store energy. The dephosphorylation of phosphocreatine, like that of ATPATP, is a highly exergonic reaction with ΔG∘′=−10.3kcal/molΔG∘′=−10.3kcal/mol: Phosphocreatine+H2O⇌creatine+PiPhosphocreatine+H2O⇌creatine+Pi ATP+H2O→ADP+PiATP+H2O→ADP+Pi Choose a reaction for the transfer of phosphate from phosphocreatine to ADPADP to generate creatine and ATPATP. ANS: P-creatine+ADP→creatine+ATP B: Calculate ΔG∘′ΔG∘′ for the reaction. Express your answer using one decimal place. C: If ΔHΔHDH = -50.0 kJkJ and ΔSΔSDS = -0.300 kJ/KkJ/K , the reaction is spontaneous below a certain temperature....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT