5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-² The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?

5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-² The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter5: Alkenes: Bonding, Nomenclature, And Properties

Section: Chapter Questions

Problem 5.31P

See similar textbooks

Similar questions

The standard Gibbs energy of the isomerization reaction of cis-2-pentene to trans-2-pentene at 400 K is -3.67 kJ mol-. Calculate the equilibrium constant of the isomerization.
At constant pressure and 25°C, what is ΔrH° for the following reaction2C2H6(g) + 7O2(g) → 4CO2(g) + H2O(l)if the complete consumption of 14.5 g of C2H6 liberates 752.3 kJ of heat energy?
What is the pH of rainwater at 25°C in which atmospheric CO2 has dissolved, producing an initial [H2CO3] of 1.28×10-5 M ? Take into account the autoionization of water.
Given that the Ksp for Ag2S is 6×10^-51, Kf=1.1×10^5 for AgCl2-, and Ka1 and Ka2 for H2S are 9.5×10^-8 and 1×10^-19, respectively, calculate the equilibrium constant for the following reaction .
If the G for a reaction is 4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the change in entropy of this reaction if H = 3.2 kcal/mol?
Calculate the equilibrium constant, Kc, of the reaction: HCO3-(aq) + HCO3-(aq) ↔ H2CO3(aq) + CO32- , Kc = ? Based on your result, do you expect this reaction to occur in the left-to-right direction?
According to Schwabe and Wagner, the heats of combustion in a constant-volume calorimeter for fumaric and maleic acids are -1337.21 kJ mol-1 and -1360.43 kJ mol-1, respectively, at approximately 25 °C. What is the enthalpy of isomerization of maleic acid into fumaric acid in kJ mol-1?
Sulfuric acid (H2SO4) is a strong acid in aqueous solution, yet the pKa of sulfuric acid is 7.6 in acetonitrile (CH3CN). Explain how this can be in terms of the relevant equilibria and the properties of the two solvents.
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10-4 △G°=19.1kJ What is the value of △G at equilibirum?
Sulfuric acid (H2SO4) is a diprotic acid where the first deprotonation is a strong acid process, and the second deprotonation is a weak acid process with Ka = 1.0 x 10-2. What is the pH of a 0.00075 M solution of sulfuric acid?
4. Anammox bacteria are known to obtain energy from the anaerobic autotrophic oxidation of one mole of NH4+ with N02- to form one mole of N2. (1) Develop an electron equivalent energy reaction for the anammox organisms. (2) Calculate ΔGr (kJ/1nol) for this reaction. (3) Calculate fs° for the anammox autotrophic reaction, assuming ε =0.4, N02- is the N source, inorganic carbon is the carbon source and Y is in g VSS/g N.
Write the chemical equations involved for the reaction of cyclohexene with cold KMnO4