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- A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 95.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH- 484. kJ AS - 1379. K 2H,0) – 21,(2) + 0,62) AG - OkJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = 1212. kJ AS Continue Submit Assignm 0 2020…Me 03, -78 °C then Zn, CH;CO2HThe standard entropies at 298 K for certain group 4A elementsare: C(s, diamond) = 2.43 J/mol-K, Si1s2 = 18.81 J/mol-K, Ge1s2 = 31.09 J/mol-K, and Sn1s2 = 51.818 J/mol-K. All but Sn have the same (diamond) structure. Howdo you account for the trend in the S° values?
- Which of the following transformations are spontaneous at room temperature and standard conditions? i) Cu(s) + Zn2*(aq) --> Zn(s) + Cu2*(aq) ii) Mg2+(aq) + Zn(s) --> Mg(s) + Zn2+(aq) iii) Zn(s) + 2 Fe3+(aq) --> Zn2+(aq) + 2 Fe2*(aq) Data: Mg2+ + 2 e-- Mg(s) Eºred = -2.36V ---> Zn2+ + 2 e- ---> Zn(s) E°r red = -0.76V %3D Cu2+ + 2 e- ---> Cu(s) Eºred = +0.34V Fe3+ + e- ---> Fe2+ E°, +0.77V red iii ii i, ii Oi ii, ii17. For which of the following highly exothermic processes would you expect AH" and AG* to be about the same? (a) 2 Al(s) + 3/2 02(g) - Al;0:(s) (c) 2 Na(s) + 2 H20(1) → 2 N2OH(aq) + H2(g) (d) 2 NO(g) - N;O(g) (e) 2 Al(s) + Fe2O;(s) - 2 Fe(s) + Al;Oa(s) (b) 2 Ha(g) + Ozl8) - 2 H;0(g)3. A particular protein heat denatures with a melting temperature Tm = 332 K with an enthalpy of unfolding, AHm = 372 kJmol-¹. (a) What is the entropy of unfolding in kJ mol-1 K-1 at Tm? (b) If ACp is 6.6 kJ mol-1 K-1, at what temperature does the free energy of unfolding (AG unfolding) have the greatest value (i.e. the native state is most stable)? (c) Calculate the value of AG and K at this temperature.
- The density of rhombic sulfur is 2.070 g cm-3 with a standard molar entropy of 31.80 J K-1 mol-1. The density of monoclinic sulfur is 1.957 g cm-3 with a standard molar entropy of 32.6 J K-1 mol-1. (a) Can an increase in temperature be expected to make monoclinic sulfur more stable than rhombic sulfur? (b) If so, at what temperature will the transition occur at 1 bar?Calculate AG°for the combustion of propane. C3H8(g) + 502(g) → 3CO2(s) + 4H20(g) Standard Thermodynamic Properties for Selected Substances Substance AH; (kJ mol-) AG; (kJ mol-1) S° (JK-1 mo Co3 2 (aq) -677.1 -527.8 -56.9 CH4(g) -74.6 -50.5 186.3 CH3OH() -239.2 -166.6 126.8 CH3OH(g) -201.0 -162.3 239.9 CCI4() -128.2 -62.5 214.4 CCIA(9) -95.7 -58.2 309.7 CHCI3() -134.1 -73.7 201.7 CHCI3(g) -103.14 -70.34 295.71 CS2() 89.70 65.27 151.34 CS2(g) 116.9 66.8 238.0 209 2 200.9 027 4DELET IEa 2 NO(g) + 02(9) → N,O.(g) Use the following reactions with known A,G° values: N204(9) + 2 NO: (g). A,G = 2.8 kJ mol -1 NO(g) + 02(9) → NO2(9). A,G =- 36.3 kJ mol- Express your answer using one decimal place. A,G° = -75.4 kJ mol Submit Prevlous Answers Completed Part B Now, calculate the A,G° for the same reaction, based on the Standard Gibbs Energies of formation: AG"NO= 87.6 kJ - mol- A,G"N,0,= 9.8 k.J - mol-1 A,G = -75.4 kJ - mol- Submit Prevloue Anewere Completed Part C Using two very different method to solve for A,G, your answers from part A and part B will be the same. Why? O The reaction is spontaneous under all conditions O Gibbs Energy is a state function O Gibbs Energy is independent of temperature O The reaction is at equilibrium under standard conditions
- P17B.9 The gas phase decomposition of ethanoic acid at 1189K proceeds by way of two parallel reactions: k, = 3.74s k, = 4.65s (1) CH,COOH → CH, + CO, (2) CH,COOH → CH,CO+ H,O (a) What is the maximum theoretical yield of the ketene CH,CO at this temperature? (b) Does the ratio of ketene to methane vary over time?Calculate the value of ΔdissolveG0 from the values of ΔdissolveH0 and ΔdissolveS0 and comment on the spontaneity of the dissolution process. ΔoplosG0/kJ mol-1 = ΔoplosH0-TΔoplosS0 = 19.69 kJ mol-1 - (298.15 K) x (80.15 x 10-3 kJ K-1 mol-1) = -4.21 kJ m comment:For the reaction X(g) + 2Y(g) = 3Z(g) K, = 2.08x10-2 at a temperature of 325 °C. Calculate the value of Kc . Express your answer numerically. View Available Hint(s) V ΑΣφ K = %3D