Calculate the equilibrium conversion and concentrations for each of the following reactions. Assume that CC,0 = 0. Part (b) and (f) are conceptual questions. (a) The liquid-phase reaction ↔ + with CA0 = CB0 = 5 mol/dm3 and KC = 1 mol/dm3 . (b) If the reaction in part (a) were a gas-phase reaction, will a constant volume or constant pressure batch reactor result in a higher conversion of A? Why? (c) The gas-phase reaction 2 ↔ is carried out in a flow reactor with no pressure drop. Pure A enters at a temperature of 400 K and 10 bar. KP (298 K) = 3 bar-1 and ΔHrxn o (298 K) = -1 kJ/mol. Neglect ∆Cp. (d) The gas-phase reaction in part (c) carried out in a constant volume batch reactor. (e) The gas-phase reaction in part (c) carried out in a constant pressure batch reactor. (f) For parts (c)-(e), which reactor(s) had the highest conversion? Why?

hope it

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= initial pressure

= final pressure = 2

= initial volume

= final volume = /4

= initial temperature = 20 c = 20 + 273 = 293 k

= final temperature = ?

using the equation