A+B--> 2C+D is a gas phase elementary reaction. A and B are loaded in equimolar proportions. Write the rate law in terms of conversion, evaluating for all constants. What are the concentrations for both products C and D when X=0.75?
The reaction given is
A +B ---> C +D
For an elementary reaction the rate of reaction will be given by
Now
Ca = Cao(1-Xa)
and for Component B
Cb = Cbo(1-Xb)
substituting these values in rate equation
Now for an elementary reaction
we have the following relation
now here gamma is nothing but the stoichiometric coefficients
gamma a and gamma b will be -1 each respectively
substiuting these vales we get
we will use these equation and substitute back in the rate equation
Now here we have equimolar proportions of both the reactants hence ratio of Cbo to Cao will be 1
Now
Xa = 0.75
let the initial concentrations of A and B we 1 and 1
Hence Cao=Cbo=1
Cc = Cco + 2*Xa = 0 + 2*0.75 = 1.5 mols
Cd = Cdo + Xa = 0 + 0.75 = 0.75 mols
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