Question

. Acetic an hydride is hydrolysed by water to form acetic acid in accordance with the equation: \left(\mathrm{CH}_{3} \mathrm{CO}\right)_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \Leftrightarrow 2 \mathrm{CH}_{3} \mathrm{COOH} In dilute aqueous solution where water is in vast excess, the reaction is irreversible and pseudo first order with respect to acetic an hydride. The variation of the pseudo first order rate constant with temperature is as follows: A batch reactor for carrying out this hydrolysis is charged with an acetic anhydride solution containing 0.60 kmol m³ at 15 °C. The specific heat and density of the solution are 3.9 kJ kg! K and 1120 kg m³, and may be taken as constant throughout the course of the reaction. The reaction is exothermic and the heat of reaction is 215,000 J molanhydride. The reactor is operated adiabatically and the desire is to achieve 85%hydrolysis of the anhydride (a)Conduct an energy balance over the reactor and calculate the adiabatic temperature rise. Assuming an average value for the rate constant (i.e. constant for the reaction),calculate the time required for the reaction via the algebraic method. Allowing the rate constant to vary with temperature, calculate the time required for the reaction using a numerical method. Comment on the difference between your answer to part (b) and (c).

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