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A(g) + B(g) C(g)
The rate law for the above reaction is:
-d[A]/dt = k[A][B]
The rate constant is 2.97×10-6 L mol-1 s-1 at 347.0°C and 5.23×10-5 L mol-1 s-1 at 555.0°C.
Use the Arrhenius equation
k = Ae-Ea/RT
part A :-Calculate Ea for this reaction.?
5.89×101 kJ/mol (i GOT THIS PART CORRECT)
PART B:- Calculate the rate constant k at 423.0°C for this reaction.?
PART C:-Calculate the pre-exponential factor A for this reaction.?
HOW TO SOLVE PART B (I GOT THE ANSWER 3.32*10^-6 BUT IT IS INCORRECT, I USED THE UNITS L/mol/s) and how to solve part C?
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