1.) 2A B + C The above reaction is run and found to follow second order kinetics

Question

1.) 2A B + C

The above reaction is run and found to follow second order kinetics with a rate constant of 1.30 x 10-3 M-1sec-1. If the initial concentration of A is 1.33 M, what is the concentration after 164 seconds?

2.) 2A B + C

Two trials of the above reaction are run with the same initial concentration of A. The first trial is performed at 25oC and the second at 35oC. If the rate constant at 25oC is 0.434 M/min, what is the rate constant in the second trial if the reaction has an activation energy of 31.3 kJ/mol?

Explanation / Answer

1)

rate constant k = 1.30 x 10-3 M-1sec-1.

initial concentration of A = 1.33 M

time = 164 sec

k = (1/t) { 1/[ A] - 1/ [A0] } for second order

1.30 x 10-3 = (1/164) { 1/[ A] - 1/ 1.33 }

[ A] = 1.0361M

concentration after 164 seconds = 1.0361 M

2) rate constant at 25oC = 0.434 M/min,

reaction has an activation energy = 31.3 kJ/mol

rate constant in the second trial = ?

log(k2/k1) =( Ea/2.303R)[1/T1-1/T2]

log(k2/0.434) =( 31.3 / 2.303 x 8.314 x 10^-3)[1/298-1/308)

k2= 0.654 M / min

rate constant in the second k2= 0.654 M / min

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