I badly need help in this can't even get past letter a:
Given the gas phase reaction: A + 2 B → R + S as first order with respect to each reactant and conducted in a constant volume batch reactor at 400K. The feed contains some inerts and initial total pressure is 4 atm. The rate of change of total pressure (P) with time in terms of P is given by:
dP/dt = 0.04[P-2.7][3-P] in atm per min
a) Determine the mole % composition of the feed.
b) What are the values and units of kA and kB in mol, Lit, min?
c) What is the half-life of A (min) and what is the total pressure at this time?
d) If the reaction is conducted at 400K and 4 atm constant pressure using the stoichiometric amounts of A and B in the feed and no inerts, what will be the new half-life of A, and what will be the % increase in total volume at this half-life?
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