Hydrazine, N2H4, is a liquid substance used in rocket fuels. Its combustion liberates 622.4 kJ of energy. For the reaction: N2H4(l) + O2(g) → N2(g) + 2 H2O (l) ∆H°rxn = -622.4 kJ a. Calculate the ∆Hf of hydrazine. b. The absolute entropy of hydrazine is 219.5 J/ K•mol, Use the standard thermodynamics value to calculate the ∆S° for the reaction. c. Use the standard enthalpy and entropy of the reaction to calculate the ∆G°. d. Use the values of ∆G° for the reaction to calculate the Gibb’s free energy of formation of hydrazine.

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. :)

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 g of the compound produced 0.213 g CO2 and 0.0310 g H2O. In another experiment, it is found that 0.103 g of the compound produces 0.0230 g NH3.What is the empirical formula of the compound? Hint: Combustion involves reacting with excess O2. Assume that all the carbon ends up in CO2 and all the hydrogen ends up in H2O. Also assume that all the nitrogen ends up in the NH3 in the second experiment.

9.20. Ammonia is oxidized with air to form nitric oxide in the first step of the production of nitric acid. Two principal reactions occur: 4 NH3 + 5 024 NO + 6 H₂O 2 NH3 + 2O₂ → N₂ + 3 H₂O A flowchart of the reactor follows. 100 mol NH3(g)/min 25°C, 8 bar 900 mol air/min 0.21 02 0.79 N₂ 150°C, 8 bar REACTOR Product gas: 700°C, 8 bar 90 mol NO/min 0000 150 mol H₂O(v)/min 716 mol N₂/min 69 mol 0₂/min ġ(kJ/min)