Calculate the change in the standard entropy of the system, ΔS°, for the synthesis of ammonia from N2(g) and H2(g) at 298 K:N2(g) + 3 H2(g)----->2 NH3(g)

Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH) and the standard molar entropy (Sº) values for diamond and graphite. Part A AGrxn= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond →Cgraphite Submit Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) O Substance Cgraphite Cdiamond μA Value AH (kJ/mol) Units 0 1.897 ? S° (J/mol. K) 5.740 2.38

Given the following reaction, calculate the standard entropy at 25oC. 2NO(g) + O2(g) 2NO2(g) (Sof NO2 = 240.1 J mol-1K-1; Sof NO = 210.8 J mol-1K-1; Sof O2 = 205.1 J mol-1K-1)

Predict which member of each of the following pairs has the greater standard entropy at 25°C: (a) Sc1s2 or Sc1g2, (b) NH31g2 or NH31aq2, (c) O21g2 or O31g2, (d) C(graphite) or C(diamond). Use Appendix C to find the standardentropy of each substance.

Calculate the standard free-energy change AG® and the equilibrium constant K, for the following reaction at 25°C. CO(9) + 2H2 (9) CH; OH(9) AG¡ (kJ/mol) Substance CO(g) H2 (9) CHOН (9) -137.2 -162.0 AG" = kJ Ky

AG (ky/mol) SUbStance / 1on so (ky/mol) -1206.9 /moi k) 92.9 • CaC03l>) -|128.8 • CaO (s) |- 635. I – 60 3.5 38.2 • CO2(9) - 393.5 - 394.4 213.7 191.5 3 H2(g) 202.7 ZNH3 ) -45.9 -16 193 • Hz (g) 202.7 223.0 -92.31 - 95. 30 186.79

A chemicai engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 42.0 °C and constant total pressure. Then, he 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 his 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. ΔΗ Ξ - 70. kJ J AS = -151. K TiCl, (g) + 2H,0(g) → Tio, (s) + 4H Cl (g) AG = || kJ Which is spontaneous? this reaction the reverse reaction neither AH = 439. kJ AS = K 4H,PO, (s) →…

Calculate the change in the molar entropy of solid sodium chloride at constant pressure (1.00 bar) during heating from 0°C to 400°C. The constant-pressure molar heat capacity of NaCl(s) – which is not constant - takes the following form. 45.94 J 16.32 x 10-3 J T. Cp,m3 K mol K2 mol

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