The elementary irreversible reaction A+B→ C is conducted in the gas-phase in an isothermal PFR. The feed enters the reactor at a pressure of 10 bar and the temperature of 650 K and consist of 30% A, 30% B and 40% inert. The conversion of A in an existing PFR is measures to be 50%. By what factor should the PFR volume used for this process be increased to achieve a conversion of 75% if there is no change in the feed stream?

Based on this diagram, answer the following questions: a) starting from a liquid mixture of 20 mol A and 80 mol B , at which T will it start to boil? b) Which would be the composition of the first vapour appeared? c) At which temperature will disappear the last liquid drop? Which will be its composition? d) How many boiling-condensation cycles would be needed for obtaining compound A with at least 90% purity? Give the composition of each vapour obtained in the process. Results: a) T ≈ 112.2 ºC, yA ≈ 0.30; b) T ≈ 115 ºC, xA ≈ 0.12; * c) 1st step: T ≈ 112.2 ºC yA ≈ 0.30 2nd step: T ≈ 108.5 ºC yA ≈ 0.422 3rd step: T ≈ 105.5 ºC yA ≈ 0.590 4th step: T ≈ 100.5ºC yA ≈ 0.720 5th step: T ≈ 97 ºC yA ≈ 0.820 6th step: T ≈ 94 ºC yA ≈ 0.865 7th step: T ≈ 92.7 ºC yA ≈ 0.925

Ammonia is to be produced from nitrogen and hydrogen. The feed is at 500 C, 10 atm at 100kmol/min. We wish to hold the reactor at isothermal conditions and at constant pressure. The conversion is expected to be 25%. a. write the balanced reaction equation b. Will the reactor require heating or cooling c. at what rate?

1. Consider a gas-phase reaction, 2A - B +C + 3D with r = kC Initially 50% A and 50% inert are present. If the pressure and temperature remain constant, determine the final volume in terms of the initial and fractional conversion.

For the gas-phase reaction A = 2B operated at 1.0 bar: Initially, the reactor contains only A, at 1.0 mol. a. Prove that the reaction coordinate (moles of A consumed) equals the following: (see attactched image) b. Make a plot of the reaction coordinate versus temperature between 200 and 400 K for exothermic reaction conditions, making use of the van’t Hoff Equation. Data: Ka = 5.0 at 298 K, ΔHrxn0 = -50.0 kJ mol-1. Neglect the ΔCp term. c. Repeat Part b for endothermic conditions. Ka = 5.0 at 298 K, ΔHrxn0 = +50.0 kJ mol-1. Neglect the ΔCp term. d. If the reaction described in part b (i.e., exothermic conditions) were operated in a simple batch reactor, would the reaction mixture’s temperature increase, decrease, or remain constant as the reaction progressed? To maximize conversion, would you recommend that heat be added to, or removed from, the reactor?

An isothermal continuous flow reactor is needed to carry out the decomposition of ethanal toproduce methane and carbon monoxide. The process takes place in the presence of nitrogen at595 K and 1.5 bar as shown below:CH3CHO → CH4 + CO The reactor used is a plug flow reactor. 1) Detailed sketch of the reactor. 2) Mechanical design

Answer the following question using the reaction coordináte diagram shown below. 280 240 E 200- E 160- 120+ 80 40- Time What is the enthalpy (AH) of the reverse reaction? A. 240 kJ B. -80 kJ C. 80 kJ D. 160 kJ Heat content (H) kilojoules