I can't seem to come up with the same answer as the book for this problem, and I don't understand where I am going wrong. I am asked to determine the rate of reaction given a balanced equation, a Temperature, and some experimental values:
The Arrhenius equation: k = Ae^-(Ea/RT)
The reaction in question is a decomposition reaction, therefore it is First Order and has a rate law of rate = k[B]
Ea = 221 kJ/mol; A = 1.2E14/s; R = 8.314 J/(mol*K); T = 673 K; [B] = .012 mol/L
By the Arrhenius equation: k = 1.2E14/s * (e^-(221 kJ/mol *1000J/kJ * molK/8.314J * 1/673K))
Simplifying the exponent: -(221000/5595.322) = -39.497 (all units cancel in the exponent)
Rewrite the Arrhenius equation: k = 1.2E14/s * e^-39.497
Simplify again: k = 1.2E14/(e^39.497)s
Divide: k = 8.43E-4/s
Substitute back into rate law: rate = 8.4E-4/s * .012 mol/L
rate = 1.01E-5 mol/L s
Now, this answer is in the correct units for a reaction of first order, and compares with the units in the answer section. However, the numerical value the book shows for the rate of reaction is 8E-4 mol/Ls, which is approximately the value I solved k for. So my question is, if anyone here can follow the algebra, have I worked this correctly and did whoever wrote the answer section in the book just not apply k to the rate law, or have I blundered somewhere?