Question

(Show all equations and calculations; No Equations & No Calculations- No Points) Part III (8 pts) 1. The rate of the reaction A +2B Chas been observed at 25'C Expt. A] (M) 0.100 0.200 0.100 IB] (M) 0.100 0.100 0.300 Initial Rate (M/s) 5.50x 10 1.65 x 10s From this data: (a) Determine the order of the reaction with respect to A. c from o.loo0,20o is tmes 2 (b) Determine the order of the reaction with respect to F hange from k 3137 (c) Write the rate law for the reaction, and give the overall reaction order kr A (d) Calculate the rate constant, and give the correct units (4 pts) 2. The rate constant of a first-order reaction is 346 102s at 298 K. What is the rate constant at 350 Kif the activation energy for the reaction is 50.2 kJ/mol? (R 8.314 J/mol-K) 나 -

Answer 1

1) A + 2B $\rightarrow$ C

Let the rate law is given by, rate = k[A]^m[B]ⁿ

where, m and n are order with respect to A and B respectively.

m+n = overall order of the reaction

k =rate constant

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d) The general formula for the unit of rate constant is M^(1-n)(time)^-1

n = order of reaction = 3, time is in Sec

Thus, unit of rate constant = M^(1-3)(Sec)^-1 = M^-2 Sec^-1

e) Let, [A] = 0.1 M

[B] = 0.1 M

rate of reaction = 5.50 x 10^-6 M/Sec

k = Rate / [A]²[B]

=( 5.50 x 10^-6 M/Sec) /(0.1)²(0.1)

= 5.5 x 10^-3 M^-2 Sec^-1