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. The first order rate constant for the decomposition of ethyl iodide by the reactionC2H5I(g) → C2H4 (g) + HI (g) at 600K is 1.60 × 105 s1. Its energy of activation is 209 kJ/mol.Calculate the rate constant of the reaction at 700K.

use the arrhenius equation .... log( k1/k2) =( EA/2.303R) [ 1/ T1 - 1/T2 ] where EA is the activation energy and k1 k2 are the respecitve rate constants and T1 AND T2 are the temperatures !!!hope u got the point !!

  • -21
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  k = Ae^-Ea/RT 
T1 = 600,T2 = 700, 
Ea = 209,k1 = 1.6*10^-5 s^-1 
k1/k2 = e^(Ea/R(1/T2 - 1/T1) 

Plug in values and solve I hope you can do that!!
  • -6
T1= 600K ,k1=1.60x10-5s-1
T2=700k ,k2=? ,Ea=209 kJ mol-1

Applying Arrhenius equation, logk2/k1= Ea/2.303R(1/T1-1/T2)
=log(1.60x10-5) + 209000 J mol-1/ 2.303x8.314 JK-1mol-1 (700-600/600x700)
=(-5+0.2041) + 2.5989 = -2.197 = 3.8030
K2=antilog3.8030=6.353x10-3 s-1
  • 39
 Dear student,

Ea = 209 kJ mol-1 = 209 x 103 J mol-1
 T1 = 600 K, k1 = 1.6x10-5 s-1
 T2 = 700 K, k2 = ? 
 R = 8.314 JK-1 mol-1
log(K2/K1) = Ea/2.303R [ (T2-T1)/T1T2]
                    =209x 10 3 /2.303 x 8.314 x [700 – 600)/ 600 x 700]
                    =2.5989
(K2/K1) = antilog 2.5989 = 397.1
K2 = 397.1 x K1= 397.1 x 1.6x10-5 s-1
K2 =6.35 x 10 -3s-1
 
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6.35*10-3
 
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Don't copy cross one.. Ans is 6.5*10^-3 s-1 Hope this help you all..😄😄

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Plz ans reply

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