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(i have the answer for b and c i only need answers for D F :- (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")
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(i have the answer for b and c i only need answers for D F :-
(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")
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