Question

The irreversible gas-phase reaction A + B ----> C is carried
out in an isothermal (400 C) constant-pressure (1 atm) batch
reactor in the presence of inerts (I). The initial gas composition
in mole fractions is given by y_{A}_{0} = 0.40;
y_{B0} = 0.40; y_{C0} = 0.10; y_{I} = 0.10.
The reaction is first-order both in A and in B with a rate
constant, k = 3.46 x10^{-2} dm^{3}mol^{-1}
s^{-1} at 400 C.

(a) Set up a stoichiometric table.

(b) Determine the time it will take for y_{C} to reach
0.20.

Answer #1

A liquid phase reaction A+B --> C+D is to be carried out in
an isothermal and well mixed batch reactor. The initial moles of A
and B are both 0.1 mole. The rate of destruction of A is
given by –rA = k*CA*CB, with k
= 6.0 L/ (mol*min). Calculate the amount of
time (in minutes) that the reaction must proceed within a 10 L
reactor in order to achieve a final concentration of A of 0.001
mol/L. Please express your answer to...

The irreversible gas-phase non-elementary reaction A + 2B
---> C takes place in an isothermal (227 C) constant-volume
batch reactor. The initial feed to the reactor consists of 40 mol%
A and 60 mol% B at a total pressure of 10 atm. Measurements of the
rate of reaction as a function of conversion yielded the following
results:
-rA (mol dm^-3 s^-1) x (1x10^8)
0.010
0.005
0.002
0.001
XA
0.0
0.2
0.4
0.6
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The reaction is zero
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drop parameter α = 0.01 kg-1, the exit conversion was found to
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(b) If the CSTR’s volume...

1. A ⇄ B + C
The above gas phase elementary reversible reaction is carried out
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When the equilibrium constant KP is 10 atm, find the
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