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The reaction A → B is conducted in an adiabatic plug flow reactor (PFR). Pure A at a concentration of 2 kmol/m3 is fed to the reactor at the rate of 0.01 m3/s and at a temperature of 500 K. If the exit conversion is 20%, then the exit temperature (in k) is (Data: Heat of reaction at 298 K = -50000 kJ/kmole of A reacted Heat capacities CPA = CPB = 100 kJ/kmole. K (may be assumed to be independent of temperature))

The reaction A → B is conducted in an adiabatic plug flow reactor (PFR). Pure A at a concentration of 2 kmol/m3 is fed to the reactor at the rate of 0.01 m3/s and at a temperature of 500 K. If the exit conversion is 20%, then the exit temperature (in k) is (Data: Heat of reaction at 298 K = -50000 kJ/kmole of A reacted Heat capacities CPA = CPB = 100 kJ/kmole. K (may be assumed to be independent of temperature)) Correct Answer 600

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An irreversible aqueous phase reaction, A + B → P, is carried out in an adiabatic mixed flow reactor. A feed containing 4 kmole/m3 of each A and B enters the reactor at 8 m3/hr. If the temperature of the exit stream is never to exceed 390 K, what is the maximum inlet feed temperature allowed?
(Data: Heat of reaction = -50 kJ/mole, Density of the reacting mixture = 1000 kg/m3, Specific heat of reacting mixture = 2 kJ/kg.K)
The above data can be assumed to be independent of temperature and composition.
Pick out the wrong statement below:
I. For the same conversion, the holding time required in a batch reactor, is always equal to the space time required in a PFR.
II. Two mixed reactors of unequal size are available for producing a specified product, formed by a homogenous second order reaction. To achieve maximum production rate, the smaller reactor should be placed in series before the larger reactor.
III. Arrehenius equation describing the effect of temperature on rate constant is given by, $${\text{K}} = {\text{A}}.{{\text{e}}^{ - \frac{{{\text{Ea}}}}{{{\text{RT}}}}}}$$
IV. The mechanism for the decomposition of CH3CHO into CH4 and CO in presence of I2 is:
CH3CHO + I2 → CH3I + HI + CO; slow
CH3I + HI → CH4 + I2; fast
Then the rate of disappearance CH3CHO is equal to K.CCH3l.CHl and acts as a catalyst.
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