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- Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 C2H4(g) 52.30 68.11 219.4 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 1. What is the value of ∆S⁰ for the catalytic hydrogenation of ethene to ethane: C2H4(g) + H2(g) → C2H6(g) + 2H2O(l) in J/K?The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.The spontaneity of the following redox reaction with investigated by determining the change in Gibbs free energy at various temperature: Cu(s)+Ag^+(aq)--> Cu^2+(aq)+Ag(s) The data from the experiment is reproduced below: T/K DeltaG/kj 277.1 88.7665 287.1 82.2055 295.4 75.8375 304.9 69.0835 312.4 67.5397 322.5 64.8381 With the use of a spreadsheet program, generate a well-labeled plot of a DeltaG vs T and write down the equation of the trendline. From the graph, determine the deltaH and deltaS of the redox reaction. Explain the meaning of the changes in enthalpy and entropy of the reaction.
- Calculate the standard Gibbs reaction energy for the reaction at 298 K, 2CH3CHO(g) + O2(g) - > 2CH3 COOH(I) Given the following data, Sm\deg (CH3CHO(g )) = 250.30 J K-1 mol-1 Sm\deg (O2(g)) = 205.10 JK -1 mol-1 Sm\deg (CH3COOH(l))=159.80~K-1~mol-1\backslash Delta fHm\deg (CH3CHO(g))=-166.20~kJ~mol-1\backslash Delta fHm\deg (O2(g)) = 0.00 kJ mol-1 \Delta fHm\ deg (CH3COOH(I)) = 484.50 kJ mol-1The standard Gibbs energy of formation of gaseous ozone at 25.0 ℃ ΔfGo, is162.3 kJ. mol-1, for standard state of 1 bar. The reaction is: 3O2 (g) ⇌ 2O3(g). Calculate the value of Kx at 2 bar.For an aqueous solution saturated in both AgCl and AgI, at 1 bar and at 298 K. The equilibrium constants for this system are given as follow: Ksp(AgCl) = 1.8*10^-10, Ksp(AgI) = 8.5*10^-17, and Kw = 1.0*10^-14. How many formalities must be given to get unique values for all the concentrations?
- Reaction KspKsp ΔH°ΔH° ΔS°ΔS° FeCO3(s)⇄Fe2+(aq)+CO32−(aq)FeCO3(s)⇄Fe2+(aq)+CO32−(aq) 3×10−113×10−11 <0<0 >0>0 MnCO3(s)⇄Mn2+(aq)+CO32−(aq)MnCO3(s)⇄Mn2+(aq)+CO32−(aq) 2×10−112×10−11 <0<0 >0 The table above lists the equilibrium constants and changes in thermodynamic properties for the dissolution of FeCO3 and MnCO3 at 25°C. The two-particle diagrams below represent saturated solutions of each compound at equilibrium. (see attached image) a.) The particle diagrams best represent that ΔH°<0ΔH°<0 because the ions from both compounds are solvated by water molecules. b.) The particle diagrams best represent that ΔH°<0ΔH°<0 because both compounds produce about the same amount of CO32−CO32− ions from the dissolution. c.) The particle diagrams best represent that ΔS°>0ΔS°>0 because both compounds produce a very small amount of ions from the dissolution. d.) The particle diagrams best represent that the molar solubility is greater for…Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?A) Calculate the standard reaction entropy at 298K of 1) Zn(s)+___Cu(aq) _____Zn(aq)+Cu (s) 2) C12H22O11(s)+12O2(g)____12CO2(g) + 11H2O(l) B) Continue the reaction entropies above with the reaction enthalpies, and calculate the standard reaction Gibbs energy at 298K. C) Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298K of the reactions above.
- The entropy of reaction at T=198.15K and a pressure of 5 bar.What is Ecell at 25°C for the reaction Mg(s) | Mg2+(2.347 M) || Sn2+(0.180 M) | Sn(s)? Report your answer to two decimal places and do not include units. Half-reaction E° (V) Mg2+ + 2e- → Mg(s) -2.37 Sn2+ + 2e- → Pb(s) -0.14Ca2+ and CO32- are dissolved in a beaker of sea water at 298 K, resulting in formation of a CaCO3precipitate:Ca2+ (aq) + CO32- (aq) ⇋ CaCO3 (s) ΔH0 = 13.44 kJ mol-1, ΔS0 = -120 J mol-1 K-1(i) Determine the direction of spontaneity under standard state conditions.(ii) Determine ΔG when [Ca2+] = 0.01 mol dm-3 and [CO32-] = 45 μmol dm-3. The activity coefficients of Ca2+ and CO32- in sea water are 0.28 and 0.21 respectively.