HomeworkLib
Question

Calculate the value of ΔG for the movement of fructose from the portal vein circulation (where...

Calculate the value of ΔG for the movement of fructose from the portal vein circulation (where its concentration is 1 mM) to the inside of a liver cell (where its concentration is 0.1 mM) at 37°C. Express your answer in units of kJ mol-1 using 2 significant figures.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

The expression for the calculation of the free energy released or consumed when the fructose molecule moves from the membrane is:

Jin AG RTIn [F) out

Where,

ΔG is the free energy change

[F]in is the concentration of the fructose inside the liver cell

[F]out is the concentration of the fructose outside the liver cell

R = 8.314 Jmol-1K-1

The conversion of kJ to J is shown below:

1 kJ = 10-3 J

So, R = 8.314* 10-3 kJmol-1K-1

T = 37 0C

The conversion of T(0C) to T(K) is shown below:

T(K) = T(0C) + 273.15

So, the temperature, T = (37 + 273.15) K = 310.15 K

Given,

[F]in = 0.1 mM

[F]out = 1 mM

So,

0.1 AG (8.314x10 kJmol K1(310.15K )ln =-5.94kJmol

Where negative sign signifies spontaneous process.

Answer upto 2 significant digits= -5.9 kJ/mol

0 0
Add a comment
Know the answer?
Add Answer to:
Calculate the value of ΔG for the movement of fructose from the portal vein circulation (where...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • The standard free energy (ΔG∘′)(ΔG∘′) of the creatine kinase reaction is −12.6 kJ⋅mol−1.−12.6 kJ⋅mol−1. The ΔGΔG...

    The standard free energy (ΔG∘′)(ΔG∘′) of the creatine kinase reaction is −12.6 kJ⋅mol−1.−12.6 kJ⋅mol−1. The ΔGΔG value of an in vitro creatine kinase reaction is −0.1 kJ⋅mol−1.−0.1 kJ⋅mol−1. At the start of the reaction, the concentration of ATP is 6 mM,6 mM, the concentration of creatine is 12 mM,12 mM, and the concentration of creatine phosphate is 25 mM.25 mM. Using the values given, calculate the starting concentration of ADP in micromolar.

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

    Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG∘: 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 the equilibrium constant K for the isomerization of glucose-1-phosphate to fructose-6-phosphate at 298 K. Express your answer numerically using two significant figures.

  • The ΔG°′ for the conversion of glucose-1-phosphate (G1P) to glucose-6-phosphate is -7.1 kJ/mol. What is the...

    The ΔG°′ for the conversion of glucose-1-phosphate (G1P) to glucose-6-phosphate is -7.1 kJ/mol. What is the ratio of the concentration of G6P to the concentration of G1P that provides a free energy change of –2.0 kJ · mol–1 at 37°C. [Express your answer in decimal form using 2 significant figures.]

  • A highly regulated reaction in glycolysis involves the addition of a second phosphate to fructose-6-phosphate, which...

    A highly regulated reaction in glycolysis involves the addition of a second phosphate to fructose-6-phosphate, which could be be written as: Fructose-6-phostphate + Pi à Fructose-1,6-bisphosphate + H2O The ∆Go’ for this reaction is +16.8 kJ/mol    In a muscle cell at 37 oC, assume the concentration of Fructose-6phosphate is 0.014 mM and the concentration of phosphate is 1 mM. a. What would be the equilibrium concentration of fructose-1,6bisphosphate under these conditions? b. What is Keq for this reaction? Show...

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

    Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG∘: reaction A:reaction B:glucose-1-phosphatefructose-6-phosphate⟶⟶glucose-6-phosphate,glucose-6-phosphate,   ΔG∘=−7.28 kJ/mol   ΔG∘=−1.67 kJ/mol Part A Calculate ΔG∘ for the isomerization of glucose-1-phosphate to fructose-6-phosphate. ΔG∘ = -5.61 kJ/mol Part B Calculate the equilibrium constant K for the isomerization of glucose-1-phosphate to fructose-6-phosphate at 298 K. Express your answer numerically using two significant figures. K = 9.6 Part C Calculate  ΔG when the concentration of glucose-1-phosphate is   10 times greater than the concentration...

  • Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 2 that has an equilibrium...

    Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 2 that has an equilibrium constant of K = 4.9×10−2. You may want to reference (Pages 861 - 865) Section 19.5 while completing this problem. Part A Express your answer using two significant figures. ΔG∘rxn = kJ Part B Express your answer using two significant figures. E∘cell = V

  • Part B: Calculate the formation constant for the formation of [Cu(NH3)4(H2O)2]2+ from [Cu(H2O)6]2+, given that ΔG∘...

    Part B: Calculate the formation constant for the formation of [Cu(NH3)4(H2O)2]2+ from [Cu(H2O)6]2+, given that ΔG∘ is −74.2kJ⋅mol−1 at 298 K. Express your answer numerically to three significant figures. Part C: Consider the formation of [Ni(en)3]2+ from [Ni(H2O)6]2+. The stepwise ΔG∘ values at 298 Kare ΔG∘1 for first step=−42.9 kJ⋅mol−1 ΔG∘2 for second step=−35.8 kJ⋅mol−1 ΔG∘3 for third step=−24.3 kJ⋅mol−1Calculate the overall formation constant (Kf) for the complex [Ni(en)3]2+. Express your answer numerically to three significant figures.

  • Calculate free energy (ΔG) for transporting 3 moles of Ca2+ from inside to outside of a...

    Calculate free energy (ΔG) for transporting 3 moles of Ca2+ from inside to outside of a typical cell. (Using Ca2+ = 1.5mM for outside the cell; [Ca2+] = 0.1 µM for inside the cell; T = 298k; R = 1.987x10^3 kcal/mol/deg; membrane potential (ΔV) = -50 mV (inside negative); Faraday constant = 23.1 kcal/V/mol).

  • Calculate the equilibrium partial pressure of manganese vapor above solid manganese at 25 ∘C if ΔG∘f...

    Calculate the equilibrium partial pressure of manganese vapor above solid manganese at 25 ∘C if ΔG∘f for gaseous manganese is 238.5 kJ/mol at 25 ∘C. Express your answer to two significant figures and include the appropriate units. pMn=?

  • 1. Use the data given to calculate the value of ΔG°rxn for the reaction at 25...

    1. Use the data given to calculate the value of ΔG°rxn for the reaction at 25 °C. 2 C(graphite) + H2(g) <---> C2H2(g) C(graphite) H2(g) C2H2(g) S° (J/mol ⋅ K) 5.74 130.68 201.0 (kJ/mol) 0 0 −226.8 Report answer to four significant figures.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT