You are a chemical engineer and need to synthesize some hydrogen fluoride from hydrogen and fluorine. You acquire 1.00 M hydrogen and 2.00 M of fluorine to combine in a closed flask. The equilibrium constant for this reaction is 1.14 x 102 at 232°C. Calculate the equilibrium concentration for each component. A Value- B Value- C Value-   Equilibrium Concentration of H2________  M Equilibrium Concentration of F2________  M Equilibrium Concentration of HF_______ M

The equilibrium constant for the reaction N₂ + O₂2NO is 1.69 × 10-³ at 2300 K. A mixture consisting of 2 mol of nitrogen and 1.0 mol of oxygen is heated to 2300 K at 1 bar and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.

(c)Explain the meaning of Azeotrope and their effect in distillation process. Describe how an Azeotrope of ethanol and water can be separated.

Using enthalpies of formation, calculate AHrxn for the reaction: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(()

Solve correctly please need all parts.

* The standard reaction enthalpy for the hydrogenation of propene is -124 KJ/mole. The standard reaction enthalpy for the combustion of propane is -2220 KJ/mole. What is the standard enthalpy of combustion (in KJ/mole) of propene given that the enthalpy of formation for liquid water is -285.5 KJ/mole? NOTE: Express answer in the NEAREST WHOLE NUMBER.

Please help me with this one as soon as you can and show all the work for the enthalpy table. I provided the problem statement and the enthalpy table I need filled out please show the work for it.

Two perfectly mixed vessels of 10 liters each and both at 1 atm and 120 °C are respectively filled with n-butanol C4H9OH and air. At time t = 0, the two vessels are via a pipe connected to each other at 120 °C and 1 atm. This pipe has a length of 10 cm and a diameter of 1 cm. No reaction occurs during the mixing of the gases. All performing gas phases are assumed to be ideal. For the calculation of the molecular diffusivity, the Fuller's equation used. How long does it take for the partial pressure of n-butanol in the air vessel to reach 0.01 atm (in h)? Hints for the second part: - at any time point (so also at t= 0) forms the formula derived in the course for equimolar counter-diffusion under steady state conditions is a good approximation for the occurring flux. - at any time holds that c(butanol, vessel 1) = 31 mol/m3 - c(butanol, vessel 2) with the two concentrations in mol/m3 answer: t = 2.45 h

Please only solve part D

ou have 24.0 grams of Fe203. How many moles of carbon dioxide can you form from the reaction above? 2 Fe203 + 3 c → 4 Fe + 3 CO2