For the reaction A + B → C, experimental data gives: doubling [A] doubles the rate; doubling [B] quadruples the rate. Determine the rate law and rate constant.
Formula Sheet
Rate = k[A]^m[B]^nArrhenius: k = Ae^(−Ea/RT)Half-life t₁/₂ = ln2/k (first order)Doubling [A] doubles the rate. What is the order with respect to A?
Doubling [B] quadruples the rate. What is the order with respect to B?
The overall order of the reaction (m + n) is:
If Rate = 0.04 mol/L·s when [A] = 0.2 M and [B] = 0.1 M, what is k? (Rate = k[A][B]²)