(c) Now consider producing m mole of methyl acetate using n mol of acetic acid (use your dataset for the values of m and n). If the reaction proceeds to equilibrium, how much methanol must be fed to get the required conversion? Note this will no longer be a stoichiometric feed composition.
solve this problem by hand calculation.
The production reaction for methyl acetate from methanol is a gas-phase
reaction that takes place in a batch reactor to equilibrium conditions. The
reaction is as follow:
CH3OH + CH3COOH <--> CH3COOCH3 + H20
a + b ↔ c d
When the reaction reaches equilibrium at the operating pressure and
temperature, the mole fractions (y) of the components satisfy the following
relation (the equilibrium constant):
yc X yd/ ya X yb = K
data we have been given is that:-
K=4.71
Methyl acetate mol:-65
Acetic acid:-87
Please do in order please please show working out :)
questions:-
(b) If the feed to the reactor is stoichiometric (contains equimolar
quantities of reactants) and no other components, calculate the
equilibrium fractional conversion to 4 s.f.(therfore fractional conversion cannot =1 as it shows "to 4.s.f")
(c) Now consider producing m mole of methyl acetate using n mol of
acetic acid (use your dataset for the values of m and n). If the
reaction proceeds to equilibrium, how much methanol must be fed to
get the required conversion? Note this will no longer be a
stoichiometric feed composition.
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Can you please answer these as well
(d) What is the molar composition of the final product in part c?
(e) Suggest a process flow diagram to get pure methyl acetate as a
product to be sold and identify the physical properties you would
need to design it.
(f) Propose a way to optimize this process and reduce waste with
relevant calculations.
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