Calculate the standard heat of reaction for the following reaction: the hydrogenation of benzene to cyclohexane. (1) C,H6(g) + 3H2(g) → C,H12(g) (2) C,H6(g) + 7}02{g) → 6CO2(g) +3H2O(1) AH; = -3287.4 kJ (3) C,H12(g) + 902 → 6CO2(g) + 6H2O(l) AH = -3949.2 kJ (4) C(s) + O2(g) → CO2(g) AH° = -393.12 kJ (5) H2(g) +}O2(g) → H2O(1l) AH = -285.58 kJ %3D Note: Unlike heats of formation, the standard state of water for heats of combustion is liquid. Standard pressure and temperature are the same 25°C, 1 atm.

For an equilibrium mixture obtained for the following reaction at 3000 K 2 CO2 (g) = 2 CO (g) + O2 (g) The partial pressures of CO2, CO and O2 are 0.6, 0.4 and 0.2 bar, respectively. (a) Calculate △Go at 3000 K for the reaction, as written (b) Calculate the pressure equilibrium constant for the reaction CO2 (g) = CO (g) + ½ O2 (g). Answer: [─60.4; 0.298]

Mn in groundwaterA ground water has the following conditions:{Mn2+ (aq)} = 1.0x10 -5pH = 7.0 (i.e., {H+ } = 1.0x10-7)Saturated with oxygen from the atmosphere: {O 2(aq)} = 2.63x10 -4T = 25 °C(a) Write the balanced equation for oxidation of reduced manganese,Mn2+ (aq), by dissolved oxygen (O 2(aq)) to generate MnO 2(s)(manganese dioxide) or MnOOH(s) (manganite), respectively.(b) Determine whether each of the above two reactions isthermodynamically favorable in the ground water. Which phase ofthe manganese oxide is more stable in the ground water?(c) If groundwater is at 5 oC, does oxidation of Mn 2+ (aq) by dissolvedoxygen to generate MnO 2(s) become more or less favorable?Calculate the saturated {Mn 2+ (aq)} assuming the water pH remainsat 7.0 and the dissolved oxygen concentration is 3.73x10 -4 M.   25C and 1 atm   Please be as detailed as possible. I want to be able to replicate. Thank you so much. :)

8. Consider the following chemical reaction: 7 4 HBr(g) + O2(g) → 2 H20(g) + 2 Br2(g) Identify the substance oxidized (SO), the substance reduced (SR), the oxidizing agent (OA) and the reducing agent (RA). SO: SR: OA: RA:

Consider the reaction: Ca(OH)2 (aq) + 2HCl(aq) → CaCl2 (s) + 2H₂O(1) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 2.04 moles of Ca(OH)2 (aq) react at standard conditions. AS⁰ Substance AH (kJ/mol) Ca(OH)2 (aq) HCl(aq) CaCl₂ (s) H₂O (1) surroundings -1002.8 -167.2 -795.8 -285.8 J/K

P4(g) + 6 Cl2(g) →4 PCI3(g) If 0.680 moles of P4 is mixed with 2.99 moles of Cl2 in a 1.58-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 454. °C. Assume 100% yield. 47.0 atm 82.1 atm 51.3 atm 103. atm O 75.2 atm

2. Consider the following reaction: CO) +=O=COz) s) Find AH (kJ/mol) of the reaction at 298 K and 1 bar (b) ›) Determine the spontaneity of the reaction in a furnace operating at 2000 K where the partial pressures of the compounds are: Compound iP (bar) CO(R) O₂(g) CO2(g) Consider that for this reaction AG2000k = -111 kJ/mol 0.05 2.00 2.50

The standard free energies of formation (AGF) of PC (g) and PCI,(g) are -286 and -325 kJ/mol, respectively. The equilibrium constant for the following reaction at 25°C equals (R8314 J/mol.K) OA 15X107 OB. 27 X 10-¹ OC 1.7 X 10 OD 8.1 X 105 D PCI, (g) PC, (g) + Cl₂(g)

Example 3: A vessel content, one mole of carbon dioxide is heated. The carbon dioxide is dissociated 1 as: CO₂ → CO + 0₂. 2 If the equilibrium constant is given as: Kp = 30 ln(T) – 240. After equilibrium occurs, the carbon monoxide mole fraction is 0.098 find the reached temperature of the mixture.

I need help with question 1 parts a-e on my homework