Consider the reaction -2NH3(2) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.1SK if the pressure of each gas is 40.57 mm Hg. ANSWER: kJ mol Consider the reaction CH (g) – H;O(g) 3H2(g) = CO(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 17.82 mm Hg. ANSWER kJ mol Consider the reaction +2HC(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of HC(g) is reduced to 14.0S mm Hg. while the pressures of H2(g) and Cl:(g) remain at 1 atm. ANSWER: kJ mol

A mixture of CO(g) and Hzlg) is produced by passing steam over hot charcoal: H,0(g) + C(s) – H, (g) +CO (g) hi See Periodic Table O See Hint Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound AG(kJ/mol) AH;(kJ/mol) SU/mol • K) H20(g) -228.6 -241.8 188.8 H20{4) -237.2 -285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 -137.2 -110.5 197.7 O2lg) 0.0 0.0 205.0 K

Consider the reaction below: A(ag) 2 B(ag) AGn = 4.00 kJ rxn A1 M solution of A was heated at 73.3 °C for several hours. After some time the concentration of A was determined. Answer the following questions: a) What is the maximum amount of work (AG) from/for this reaction when [A] = 0.96 M? AG(kJ) number (rtol=0.05, atol=1e-08) b) What is the concentration of B when AG = –3.80 kJ? Вм — number (rtol=0.03, atol=1e-08) c) Determine Q when AG = -8.00 kJ? number (rtol=0.03, atol=1e-08) d) If the equilibrium mixture contains [A] = 0.39 M at 165.5 °C. What is AH° and AS° of this reaction? AHkJ/mol) number (rtol=0.02, atol=1e-08) (J/mol.K) number (rtol=0.03, atol=1e-08)

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 59.0 °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 = 852. kJ J AS = 2645. K Al, 0, (s) + 2Fe(s) → 2A1(s) + Fe,0, (s) AG = | kJ Which is spontaneous? this reaction the reverse reaction neither