Σ *00 Given the information A +B 2D AH° = .HV 793.7 kJ AH° = 424.0 kJ AS = 293.0 J/K %3D AS = -214.O J/K %3D calculate AG at 298 K for the reaction A +B 2C %3D = DV ツ 11/8 0:8 F12 PrtScr Insert Delete F10 F11 F7 F8 F5 F4 Backspa 78 %24 0O 5. 7. H. MI
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- When nitric acid is produced industrially, nitrogen monoxide, NO, is first formed at high temperature. Bakefetr reacts NO on cooling further with oxygen to nitrogen dioxide: 2 NO(g) + O2 ⇌ 2 NO2 (g) Table 1: Thermodynamic data at 25°C. Bond ΔfHom Som Cop,m NO(g) 90.25 210.76 29.34 O2(g) 0.00 205.14 29.36 NO2(g) 33.18 240.06 37.20 1) Calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG25o, for reaction (1) at 25°C from the data in Table 1 2) Calculate (with all relevant intermediate calculations) the equilibrium constant K25, for reaction (1) at 25°C. 3) Industrially, however, the reaction does not proceed at 25°C but at 500°C. Therefore, calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG500o, for reaction (1) at 500°C under the assumption that the standard molar heat capacities, Cop, in Table 1 are independent of temperature in the interval [25°C, 500°C]Calculate ΔS^0reaction in J/mol at 298.15 K givenFe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)ΔS^0reaction=ΣnS^0Products−ΣnS^0Reactants Substance ΔG^0/f (kJ/mol) ΔH^0/f (kJ/mol) S^0 298K (J/mol K) Fe2O3(s) -742.2 -824.2 87.40 H2(g) 0 0 130.7 Fe(s) 0 0 27.3 H2O(l) -237.1 -285.83 70.0 ANSWER CHOICES: a) 16.7 b) -214.9 c) none of these d) 24.8 e) -134.38What is ΔG0 (in units of J) for the following reaction at 298K? O2(g) + 4H+(aq) +4Fe2+(aq) → 4Fe3+(aq) + 2H2O(l) E0cell = 0.04 V ΔG0 = –nFE0cell = –RT ln(K) R = 8.314 J/mol K F = 96,485 C / mol e- Answer in the form 1.23E4 and with units of J
- 10. The thermodynamic functions for the generic reaction A+B=>C at 25oC are: ΔH=-35.7 kJ/mole; ΔS=-6.95 J/mole*K Calculate ΔG in kJ/mole Group of answer choices 146 -37.7 -35.5 -33.6 2036If a plot of ln(Ksp) vs. T gives a straight line with slope equal to 2.4 × 103 K and y-intercept equal to -7.4, what is ΔS° for the process? −290 J/mol −62 J/mol·K −20. kJ/mol −890 kJ/mol·KCarbon dioxide from the atmosphere "weathers," or dissolves, limestone (CaCO3) by the reactionCaCO3(s) + CO2(g) + H2O(ℓ) → Ca2+(aq) + 2HCO3-(aq)Obtain ΔH° for this reaction using the following data:ΔH°(CaCO3(s)) = -1206.9 kJΔH°(CO2(g)) = -393.5 kJΔH°(H2O(ℓ)) = -285.8 kJΔH°(Ca2+(aq)) = -542.8 kJΔH°( HCO3-(aq)) = -692.0 kJ
- Calculate the Delta Hrxn for the following reaction: C(s)+O2(g)--> CO2(g) DeltaHrxn=-393.5 kJ H2(g)+1/2O2(g)--> H2O (l) DeltaHrxn=-285.8 kJ C5H12(g)+8O2 (g)--> 5CO2(g) +6H2O(l) DeltaHrxn=-3536 kJ 10C(s)+12H2(g)-->2C5H12(g) DeltaHrxn=??????Calculate ΔG0reaction in kJ/mol at 298.15 K givenFe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)ΔG^0reaction=ΣnΔG0Products−ΣnΔG0Reactants Substance ΔG0f (kJ/mol) ΔH0f(kJ/mol) S0298K (J/mol K) Fe2O3(s)Fe2O3(s) -742.2 -824.2 87.40 H2(g)H2(g) 0 0 130.7 Fe(s)Fe(s) 0 0 27.3 H2O(l)H2O(l) -237.1 -285.83 70.0 answer choices: a) 30.9 b)175.2 c)none of these d)158.7 e)-622.58If a plot of Ksp vs. T gives a straight line with slope equal to 7.9 × 103 K and y-intercept equal to 9.8, what is ΔH° for the process? 0.081 kJ/mol -66 kJ/mol 1.2 kJ/mol -950 kJ/mol
- A system goes from state 1 to state 2 and back to state 1. (a) Is ∆E the same in magnitude for both the forward and reverse processes?Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)The oxidation of glucose to CO2 and water is a major source of energyin aerobic organisms. It is a reaction favored mainly by a large negativeenthalpy change. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(1) ΔH ° = -2816 kJ/mol ΔS ° = +181 J/mol • K(a) At 37 °C, what is the value for ΔG° ?(b) In the overall reaction of aerobic metabolism of glucose, 32 moles ofATP are produced from ADP for every mole of glucose oxidized. Calculatethe standard state free energy change for the overall reaction whenglucose oxidation is coupled to the formation of ATP at 37 °C.(c) What is the efficiency of the process in terms of the percentage of theavailable free energy change captured in ATP?