Question

Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free...

Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG°:

glucose-1-phosphate ⟶ glucose-6-phosphate ΔG° = −7.28 kJ/mol

fructose-6-phosphate ⟶ glucose-6-phosphate ΔG° = −1.67 kJ/mol

3.1 Calculate ΔG° for the isomerization of glucose-1-phosphate to fructose-6-phosphate. [ANSWER = -5.61 kJ/mol]
3.2 Calculate the equilibrium constant K for the isomerization of glucose-1-phosphate to fructose-6-phosphate at 298K. [ANSWER = 9.62 ]
3.3. Suppose you dissolve fructose-6-phosphate in water to prepare a 0.1 M solution. What are the concentrations of fructose-6-phosphate and glucose-1-phosphate at equilibrium?

I JUST NEED PART 3.3

Homework Answers

Answer #1

fructose -6-phosphate   ---> glucose -6-phosphate   , dG == - 1.67 KJ/mol = -1670 J/mol

we have relation dGo = -RT ln Keq

   - 1670 J/mol = - 8.314 J/molK x 298 K x ln Keq

Keq = exp ( 1670 /8.314 x 298)   = 1.96

At equilibrium fructose-1-6-phosphate concentration = 0.1-X ,   

Glucose-6-phosphate = X

we have Keq = [Glucose-6-phosphate] / [fructose-6-phosphate]

1.96    = ( X) / ( 0.1-X)

X = 0.066

hence at equilibrium glucose -6-phosphate concentration = 0.066 M

fructose -6-phopshate concentration = 0.1-0.066 = 0.034 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
reaction A: glucose-1-phosphate ⟶ glucose-6-phosphate ΔG∘=−7.28 kJ/mol reaction B: fructose-6-phosphate ⟶glucose-6-phosphate, ΔG∘=−1.67 kJ/mol Calculate ΔG∘ for...
reaction A: glucose-1-phosphate ⟶ glucose-6-phosphate ΔG∘=−7.28 kJ/mol reaction B: fructose-6-phosphate ⟶glucose-6-phosphate, ΔG∘=−1.67 kJ/mol Calculate ΔG∘ for the isomerization of glucose-1-phosphate to fructose-6-phosphate. Express your answer with the appropriate units.
For the isomerization of glucose-1-phosphate to glucose-6-phosphate, the ΔG°′ = -7.28 (correct?). [Express your answer in...
For the isomerization of glucose-1-phosphate to glucose-6-phosphate, the ΔG°′ = -7.28 (correct?). [Express your answer in kJ/mol using 2 significant figures.] the tolerance is +/-2% At 37°C and concentrations of 5 mM glucose-6-phosphate and 0.1 mM glucose-1-phosphate, the ΔG = . [Express your answer in kJ/mol using 2 significant figures.] the tolerance is +/-2% Under these differing conditions, the isomerization of G1P to G6P is spontaneous under the 25C or 37C? Phosphoenolpyruvate Delta G = −61.9 1,3-Bisphosphoglycerate −49.4 ATP →...
A. Using given data, calculate the change in Gibbs free energy for each of the following...
A. Using given data, calculate the change in Gibbs free energy for each of the following reactions. In each case indicate whether the reaction is spontaneous at 298K under standard conditions. 2H2O2(l)→2H2O(l)+O2(g) Gibbs free energy for H2O2(l) is -120.4kJ/mol Gibbs free energy for H2O(l) is -237.13kJ/mol B. A certain reaction has ΔH∘ = + 35.4 kJ and ΔS∘ = 85.0 J/K . Calculate ΔG∘ for the reaction at 298 K. Is the reaction spontaneous at 298K under standard conditions?
Many metabolic reactions are coupled reaction. Such as the first step in glycolysis drawn below: Glucose...
Many metabolic reactions are coupled reaction. Such as the first step in glycolysis drawn below: Glucose + Pi ↔ glucose-6-phosphate + H2O a. The ΔG°’ is 14 kJ•mol-1. What is the ratio of [G6P]/[glucose][Pi] at equilibrium at 25°C? b. The above reaction is coupled to the hydrolysis of ATP. In muscle cells at 37°C, the steady-state ratio of [ATP]/[ADP] is 12 & the ΔG°’ for ATP hydrolysis is -30.5 kJ•mol-1. Assuming that glucose and G6P achieve equilibrium values in muscle...
Standard Free Energy of Hydrolysis, ∆ G o', of some organophosphate compounds (phosphate isreleased as one...
Standard Free Energy of Hydrolysis, ∆ G o', of some organophosphate compounds (phosphate isreleased as one of the products of hydrolysis)                                     Compound kJ/mol phosphoenolpyruvate -61.9 carbamyl phosphate -51.4 creatine phosphate -43.1 acetyl phosphate -42.2 ATP (to ADP) -30.5 Glucose-1-phosphate -20.9 Glucose-6-phosphate -13.8 Glycerol-3-phosphate -9.2 Use the table in the above table to calculate the ∆G o' (in kJ/mol) for the following reaction: ATP +  glucose --------> ADP  +  glucose-6-phosphate
To answer this question, please reference the Problem Solving Video: Free Energy, ATP, and Creatine in...
To answer this question, please reference the Problem Solving Video: Free Energy, ATP, and Creatine in Resting Muscles. Suppose a sprinter's muscle tissue contains creatine phosphate at a concentration of 120 mM after dietary supplementation. The sprinter's muscle tissue also contains 4 mM ATP, 0.013 mM ADP, and 13 mM creatine. Use the table of the standard free energies of hydrolysis of phosphorylated compounds and the given concentrations to calculate the free energy change, ΔG, of the creatine kinase reaction...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following reaction? Cgraphite ->  Cdiamond b. Is the diamond thermodynamically stable relative to graphite at 298 K? c. What is the change of Gibbs free energy of diamond when it is compressed isothermally from 1 atm to 1000 atm at 298 K? d. Assuming that graphite and diamond are incompressible, calculate the pressure at which the two exist in equilibrium at 298 K. e....
Calculate the non standard Gibbs Free Energy change, ΔG at 250C for the following reaction with...
Calculate the non standard Gibbs Free Energy change, ΔG at 250C for the following reaction with the indicated concentrations. Zn + 2Ag+ (0.30M) → 2Ag + Zn2+ (0.50M) Remember you'll need to calculate both the standard and non standard cell potential Ecell. Remember ΔG0 = − nFE0cell  and a similar equation for the NONstandard value ΔG = −nFEcell Here are the standard reduction potentials: Zn2+/ Zn: - 0.763V Ag+/ Ag: + 0.799V Answer in kJ to 3SF including signs as needed...
1) Given the following thermochemical reaction and thermodynamic data, find Gibbs Free Energy, ΔG, and determine...
1) Given the following thermochemical reaction and thermodynamic data, find Gibbs Free Energy, ΔG, and determine if the reaction is spontaneous or non-spontaneous at 25 °C? N2(g) + 3H2(g) → 2NH3(g) ΔH = -91.8 kJ ΔS[N2] = 191 J / mol · K, ΔS[H2] = 131 J / mol · K, and ΔS[NH3] = 193 J / mol · K a.98.3 kJ; Non-Spontaneous b.-98.3 kJ; Spontaneous c.32.7 kJ; Non-Spontaneous d.ΔG = -32.7 kJ; Spontaneous 2) What is the oxidation number...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI (b)2 NO(g) + O2(g)           2 NO2(g) (c)N2(g) + 3 H2(g)           2 NH3(g) (d) CO(g) + NO2(g)           CO2(g) + NO(g) (e) 2 CO(g) + O2(g)             2 CO2(g) 2.    Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O2(g)                  CO(g) (b) Zn2+(aq) + H2S(g)               ZnS(s) + 2 H+(aq) (c) HCl(g) + H2O()                  H3O+(aq) + Cl–(aq) (d)H2(g) +  O2(g)                   H2O(g) 3.         Which of the following is more likely to precipitate the hydroxide ion? (a)...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT