(a)
Interpretation:
The equilibrium constant for the reaction at
Concept introduction:
The change in standard free energy is given by an expression shown below.
Where,
•
•
•
•
•
(b)
Interpretation:
The standard free-energy difference between starting materials and products for a reaction that has an equilibrium constant of
Concept introduction:
The change in standard free energy is given by an expression shown below.
Where,
•
•
•
•
•
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Organic Chemistry
- 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).arrow_forwardAnother step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forwarda Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?arrow_forward
- The acid dissociation constant for a weak acid HX at 25°C is 1.9 10–6. Calculate the free energy of formation for X–(aq) at 25°C. The standard free energies of HX(aq) and H+(aq) at 25°C are –245.4 kJ/mol and 0, respectively.arrow_forwardAn important reaction in the production of energy from sugars (glycolysis) is the reduction of pyruvate to lactate by NADH. pyruvate + NADH + H+(aq) → lactate + NAD+ ΔrG°′ = ? Given the following reduction potentials, NAD+ + H+ + 2e− → NADH Ε°′ = −0.320 V pyruvate + 2H+ + 2e− → lactate Ε°′ = −0.190 V calculate the standard Gibbs free energy (at pH 7) for the reduction of pyruvate to lactate by NADH. (ΔrG°′ = −nFE°′; F = 96485 C/mol electrons)arrow_forward2b which determines whether a reaction is spontaneous. the net free energy change of the reaction or the activation energy of the reactionarrow_forward
- From the standard molar enthalpy of combustion of pentane at 298 K, calculate the value of Δr A° for the process. (For this reaction, ΔrH° = −3508.8 kJ·mol−1 and ΔrS° = −416.1 J·K−1·mol−1.)arrow_forwardEstimate the pH of an aqueous solution of sodium hydrogenoxalate.Under what conditions is this estimate reasonably reliable?arrow_forwardIf the equilibrium constant of a reaction is Keq = 9.3 × 103 at 900 °C, what is the change in Gibbs free energy for this reaction (in kJ mol–1) at the indicated temperature? R = 8.314 J K–1 mol–1arrow_forward
- Calculate the standard Gibbs free energy of the reaction, ΔG∘rxn. The standard enthalpy of the reaction, ΔH∘rxn, is −44.2 kJ⋅mol−1. C2H4(g)= 68.4 H2O(l)= -237.1 C2H5OH(l)= -166.6arrow_forwardUsing the thermodynamic informationn, claculate the standard reaction free energy of the following chemical reaction: Fe2O3(s)+3H2(g)---> 2Fe(s)+3H2O(l)arrow_forwardThe standard free energy of formation, DGf°, of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O2(g) ↔ 2O(g)arrow_forward
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