(a)
Interpretation:
The values of
The given reaction is,
The oxidation of magnetite to hematite:
(b)
Interpretation:
The values of
The given reaction is,
The dissolution of
(c)
Interpretation:
The values of
The given reaction is,
The dimerization of
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Chemical Principles: The Quest for Insight
- Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forwardIn a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.arrow_forward
- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)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_forwardWrite the chemical equation for the standard molar enthalpy of formation of nitromethane, CH3NO2.arrow_forward
- a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq. A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species. You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?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_forwardWhat is the relationship between the standard free energy change and the equilibrium constant of the reaction?arrow_forward
- Estimate the value of the equilibrium constant at 690 K for each of the following reactions using thermodynamic data from the appendix. Part A 2NO2(g)⇌N2O4(g) ΔH∘f for N2O4(g) is 9.16 kJ/mol .arrow_forwardGiven that the standard enthalpy of formation of HCl(aq) is −167 kJ mol−1, what is the value of ΔfH⦵(Cl−, aq)?arrow_forwardCalculate the standard enthalpy of solution of AgCl(s) in water from the enthalpies of formation of the solid and the aqueous ions.arrow_forward
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