CBSE Class 12-science Answered
for decomposition reaction the value of RAR constant K at two different temperature are given below-
K1=2.15*10Lmol s at 650K
k2=2.39*10Lmol s at 700K
calculate the value of activation energy for this reaction(R=8.314)
Asked by Shomyajit Misra Misra | 06 May, 2014, 09:07: PM
Expert Answer
Solution:
The Arrhenius equation is:
log k2/k1 = Ea [ T2 - T1/T1T2]
2.303R
k 1 = 2.15 x10-8molL-1s-1
k 2 = 2.39 x 10-9molL-1s-1
T1 = 650 K
T2 = 700K
Substititing the values,
log (2.39 x 10-9/2.15 x10-8) = Ea [ 700 - 650/650x700]
2.303 x 8.314
1.046 = Ea [700 - 650/650x700]
2.303 x 8.314
Ea = 1.046 x 2.303 x 8.314 x 650 x 700 = 182254Jmol-1 = 182.254kJmol-1
50
Answered by Vaibhav Chavan | 07 May, 2014, 09:17: AM
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