12. The AvapH for benzene at 298 K is 33.92 kJ mol-¹ and at 353 K is 30.72 kJ mol¹¹. If Cp for benzene gas is 82.44 J K-¹ mol-¹ at 298 K, calculate Cp for liquid benzene. Note any approximations that you make.
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- NI3 decomposes as shown below: 2 Nl3(s) → N2(g) + 3 I2(g) Use the thermochemical information given below to calculate the standard Gibbs energy change (in kJ mol¬1) of this reaction at 298.15 K. NI3(s) N2(2) 2(g). AH;° (kJ mol-1) S° (J mol-1K-1) 287.0 62.40 230.0 191.6 260.7 O-161.1 O -387.0 O +513.7 +119.0 O -540.0For CaF2(s) Ca²+ (aq) + 2 F (aq) + 2 F (aq), K = 3.9 X 10¹ at 25 °C and the standard Gibbs energy of formation of CaF2() is -1167 kJ mol¹¹. Calculate the standard Gibbs energy formation of CaF2(aq) in kJ mol A. -976 B. -1108 C. -1461What is the A,G for the following reaction (in kJ mol ¹) at 298 K? 2 Si (s) + 3 H2(g) Si₂H6 (g) 1 The conditions for this reaction are: PH2 = 1.21 bar PsizH6 = 0.5 bar. You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass. Please use the method of Gibbs energy of formation to calculate ArG" if needed. For partial credit, enter the value of "Q" for this reaction. Answer:
- Consider the reaction: N₂(g) + 3H2(g) = 2NH3(g) AG°f (NH3) = -15.73kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) Report your answer as a whole number (no places past the decimal point).the equilibrium constant for the reaction at 385 K is 2.78·10-4. Calculate the equilibrium constant for that reaction at a temperature of 345 K, when the reaction's ΔH° = 41 kJmol-1. ΔH° is assumed to be independent of temperatureFor the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium? ....... J/mol The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 68 oC is Keq = 401,568. (b) What is the standard reaction Gibbs energy of this reaction?.....J/mol
- For the system ΔΗ = -9.4 kJ H₂(g) + 2(g) 2HI(g) K = 62.5 at 800 K. "Predict the direction of the shift of the equilibrium position at 600 K."4. Titanium (IV) oxide is converted to titanium carbide with carbon at a high temperature. TIO2(s) + 3C(s)→ 2C0(g) + TiC(s) Substance AG(kJ/mol) at 727°C TIO2(s) C(s) TiC(s) CO(g) -757.8 -162.6 -200.2 Calculate the free Gibbs energy and equilibrium constant at 727°C. b. Is this reaction product favored at equilibrium at this temperature? Explain your answer How can the reactant or product concentrations be adjusted for the reaction to be a. C. spontaneous at 727°C?1. The equilibrium constant of the reaction 2 C3H5 (g) = C2H4 (g) + C4H8 (g) is found to fit the expression ln K = - 1.04 - (1088 / T) + (1.51 x 105 / T^2 ) between 300 K and 600 K. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K. [2.77 kJ mol-1 ; -16.5 kJ K-1 mol-1 ]
- 3. Initially, 0.075 mol CH3OH(g) and 0.025 mol NOCI (g) was mixed at 25°C. At equilibrium, it was found that 0.005 mol CH3NO2(g) was present. The reaction involved is shown below. CH3OH(g) + NOCIl(g) = HCl(g) + CH3NO2(g) Calculate the standard molar Gibbs free energy of the reaction, ArxnG(J/mol).One of the most extensively studied reactions of industrial chemistry is the synthesis of ammonia, for its successful operation helps to govern the efficiency of the entire economy. The standard Gibbs energy of formation of NH3(g) is -16.5 kJ mol-1, at 298 K. What is the reaction Gibbs energywhen the partial pressure of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar, and 4.0 bar, respectively?What is the spontaneous direction of the reaction in this case?Calcium oxide can decompose into calcium and oxygen according to 2CaO(s)2Ca(s) + O2(g) Calculate the standard Gibbs energy change for this at 298 K given that At(CaO(s)) = -635,1 kJ mol ¹, S(CaO(s)) = 39.7 J mol¹K¹ AP(Ca(s)) = 0, S(Ca(s)) = 41.4 J mor¹ K¹, AP(O₂(g)) = 0, and S(O2(g)) = 205 J mol¹ K¹ Answer in kJ mol