K $=4\mathrm{.}73$

Methyl acetate $=68$

Acetic acid $=87$

Design an excel file for the material balance process.

Do these questions in the form of a table for example a mass balance table and calculate.

Task $2$:

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:

$C{H}_{3}OH+C{H}_3\frac{C}{O}OHharrC{H}_3\frac{C}{O}OC{H}_3+H_{2}O$

$a+$bharrc,$d$

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$)$:

$\frac{y_c{y}_d}{y_a{y}_b}=K,(K$ from dataset$)$

$($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$.$

$($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.