Question

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. Trial [A] (M) 0.210 B] (M) Rate (M/s) 0.370 0.0218 0.740 0.0218 0.370 0.0872 A +2BC+D 0.210 0.420 Units

Answer 1

A + 2B — > C +D Rate of the reaction - Krai[B]" - ③ where, k=mate constant of the reaction X & B = Order of the reaction with respect to reactant A and B [B] (M) Trial [^] (m) 0. 370 Rate (m/s) 0.0218 0.0218 0.0872 0.210 0.210 0.420 0.740 0.370 From trial-1 - Rate (Y) = K[0.210] [0.370] => 0.0218 = K[0.210]*[0.3707 — From trial-2 Rate (m2) = { [0.210][0.74078 ->0.0218 = K [0.210][0.74078_ @ From trial-3 Rate (n 3) = K[0.420][0.370] => 0.0872 = K[0:420]4[0.3.70] P__PID

From 9 - 0.0218 0.0218 , we get k 10.21074 [0.370] B K [0.210] [0.740] => 1 = 10.370] 0.0872 => 1 = [0.740] => 1 = 28 | => B = 0 From , we get - 0.0872 k[0.420]–[0.370] 0.0218 - k{0.210] [0.370]ß => 4 = 24 => 22 = 22 -> X = 2 From ② , we get - nate (%) = K[A Trate of the reaction = K[A]² Putting the value of a and ß in equ ® 0.0218 Msta k [0.210 (m)] ² [0.370(m)] ° 0.0218 M 5' NO 1B-D L => K= 10.210) 2 M2 => [k=0.494M's in 0.5M"'s-1