The rate constant for the first order decomposition of H2O2 is given by the following equation:
log k = 14.34 - 1.25 x 104 K/T
Calculate Ea for this reaction and at what temperature will its half-period be 256 minutes?
Arrhenius equation is given by,
k= Ae -Ea/RT
⇒In k = In A - Ea/RT
⇒In k = Log A - Ea/RT
⇒ Log k = Log A - Ea/2.303RT (i)
The given equation is
Log k = 14.34 - 1.25 104 K/T (ii)
From equation (i) and (ii), we obtain
Ea/2.303RT = 1.25 104 K/T
⇒ Ea =1.25 × 104K × 2.303 × R
= 1.25 × 104K × 2.303 × 8.314 J K - 1mol - 1
= 239339.3 J mol - 1 (approximately)
= 239.34 kJ mol - 1
Also, when t1/2= 256 minutes,
k = 0.693 / t1/2
= 0.693 / 256
= 2.707 × 10 - 3 min - 1
= 4.51 × 10 - 5s - 1
It is also given that, log k= 14.34 - 1.25 × 104K/T
= 668.95 K
= 669 K (approximately)
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Welcome to the NCERT Solutions for Class 12 Chemistry - Chapter . This page offers a step-by-step solution to the specific question from Excercise 2 , Question 27: The rate constant for the first order decomposition of H2O2 is given by the following equation: l....
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