SATHEE: Chemical Kinetics Question 349

Chemical Kinetics Question 349

Question: The rate coefficient (K) for a particular reactions is $1.3 \times 10^{- 4} M^{- 1} s^{- 1}$ at $100^{\circ} C$ , and $1.3 \times 10^{- 3} M^{- 1} s^{- 1}$ at $150^{\circ} C$ . What is the energy of activation $(E_{a})$ (in kJ) for this reaction- (R = molar gas constant $= 8.314 J K^{- 1} m o l^{- 1}$ )

Options:

A) 16

B) 60

C) 99

D) 132

Show Answer

Answer:

Correct Answer: B

Solution:

[b] According to Arrhenius equation $\log \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$\log \frac{1.3 \times 10^{- 3}}{1.3 \times 10^{- 4}} = \frac{E_{a}}{2.303 \times 8.314} [\frac{1}{373} - \frac{1}{423}]$

$I = \frac{E_{a}}{2.303 \times 8.314} [\frac{1}{373} - \frac{1}{423}]$

$E_{a} = 60 k J / m o l$

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Chemical Kinetics Question 349

Question: The rate coefficient (K) for a particular reactions is 1.3×10−4M−1s−1 at 100∘C , and 1.3×10−3M−1s−1 at 150∘C . What is the energy of activation (Ea) (in kJ) for this reaction- (R = molar gas constant =8.314JK−1mol−1 )

Options:

Answer:

Solution:

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