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?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 7QRT

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Consider The Following Reaction: CaCO3(S) + 2HCl(Aq) = CaCl2(Aq) + H2O(L) + CO2(G) Write down the quation of the equilibrium constant kc for this reaction
Consider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (a)Concentration of CH3OH increases (b)H2O is removed from the reaction (c)Reaction is heated
Consider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 cal Indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (d)How does the equilibrium constant (Keq) change when temperature is decreased?
A reaction has AS>0 and AH>0. Which statement about this reaction must be correct? (A) If carried out in a well-insulated flask, the temperature of the reaction mixture will decrease. (B) It will occur spontancously at 298 K and 1 atm pressure. (C) As the temperature is raised, Keq for this reaction decreases. (D) The reaction has more moles of products than it has moles of reactants.
When ethyl acetate in dilute aqueous solution is heated in the presence of a small amount of acid, it decomposes to acetic acid and ethanol according to the equation CH;COOC;Hs + H;0 -> CH3COOH + C2HSOH Since the reaction takes place in dilute solution, the quantity of water present is so great that the loss of the small amount which combines with ethyl acetate produces no appreciable change in the total amount. Hence, of the reacting substances, only ethyl acetate suffers a measurable change in concentration. A chemical reaction of this sort, in which the concentration of only one reaction substance changes, is called a first-order reaction. It is a law of physical chemistry that the rate at which a substance is being used up in a first order reaction is proportional to the amount of that substance instantaneously present. If the initial concentration of ethyl acetate is Co, find the expression for its concentration at any time t.
At -119 °C, Keq = 0.472 for the reaction: (a) What is the value of Keq for the reaction NOBr(g) NO(g) + 1/2 Br₂(g)? = 2.12 (b) What is the value of Keq for the reaction 2 NO(g) + Br₂(g) = 2 NOBr(g)? Keq=0.944 NO(g) + 1/2 Br₂(g) = NOBr(g) |x Keq=1.06 (c) What is the value of Keq for the reaction 2 NOBr(g) = 2 NO(g) + Br₂(g)? X
Consider the reaction: 2 NH3(g) N₂(g) + 3H₂(g). At T = 740 K, the equilibrium constant Kc for this reaction is Kc = 10. What is the correct form of the equilibrium constant Kc for this reaction? (A) Kc = [N₂] [H₂]³ (B) Kc (C) Kc = (D) Kc = (E) Kc - 2[NH3] [N₂]+3 [H₂] [N₂] +3 [H₂] 2[NH3] 2 [NH3] [N₂] [H₂] ³ 13 [N₂] [H₂] ³ [NH3]²
(a) Calculate the value of Kc for the reaction: PCl5 (g) PCl3 (g) + Cl2 (g) ΔH = Positive Given that when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3container the amount of PCl5 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: Increasing temperature Lowering the concentration of chlorine (Cl2) Addition of a catalyst
The value of K for aniline, C6H5NH₂, is 7.40×10-10. Write the equation for the reaction that goes with this equilibrium constant. It is not necessary to include states such as (aq) or (1). +
(a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at 127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction. (b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.
The standard free energy change for the reaction catalyzed by phosphoglucomutase is -7.1kJ/mol, (a) Calculate the equilibrium constant for the reaction, (b) Calculate ΔG at 37°C when the concentration of glucose-1-phosphate is 1-mM and the concentration of glucose-6-phosphate is 25-mM, (c) Is the reaction spontaneous under these conditions?