(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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ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.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_forwardDetermine 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_forward
- The major industrial use of hydrogen is in the production of ammonia by the Haber process: 3H2(g)+N2(g)2NH3(g) a. Using data from Appendix 4, calculate H, S, and G for the Haber process reaction. b. Is the reaction spontaneous at standard conditions? c. At what temperatures is the reaction spontaneous at standard conditions? Assume H and S do not depend on temperature.arrow_forwardFrom the data given in Appendix I, determine the standard enthalpy change and the standard free energy change for each of the following reactions: (a) BF3(g)+3H2O(l)B(OH)3(s)+3HF(g) (b) BCl3(g)+3H2O(l)B(OH)3+3HCl(g) (c) B2H6(g)+6H2O(l)2B(OH)3(s)+6H2(g)arrow_forwardIn the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?arrow_forward
- What information can be determined from G for a reaction? Does one get the same information from G, the standard free energy change? G allows determination of the equilibrium constant K for a reaction. How? How can one estimate the value of K at temperatures other than 25C for a reaction? How can one estimate the temperature where K = 1 for a reaction? Do all reactions have a specific temperature where K = 1?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
- (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.arrow_forwardA 5.00 g-sample of KOH at 25.0 C was added to 100.0 g of H2O(l) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH is a thermodynamically favorable process? A. The forces between the ions and the water molecules are stronger than the forces between water molecules, thus, delta H < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus delta S > 0. Therefore, delta G < 0. B. The energy require to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus delta H < 0. Also, the ions become widely dispersed as KOH(s) dissolved, thus delta S > 0. Therefore, delta G < 0. C. The average kinetic energy of the particles increases, resulting in delta H > 0. Also, the…arrow_forwardWhat is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Submit AGixn = 6.24. 10¹¹ Part B AGrxn= xa Submit Part C μÅ Xb b Teq = Previous Answers X Incorrect; Try Again; 5 attempts remaining Enter your answer with a different unit type. Review a list of acceptable units. What is the Gibbs free energy for this reaction at 5975 K ? Assume that AH and AS do not change with temperature. Express your answer to two decimal places and include the appropriate units. ► View Available Hint(s) Value μА Value . μA X.10n J K X Units At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Units ? ?arrow_forward
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