the rate constant for first order decomposition if certain reaction is described by the equation log k = 9.27-7.2×10^-3K/T the activation energy of reaction is

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Q. The rate constant for the decomposition of a certain reaction is described by the equation

l o g k (s^{- 1}) = 14 - \frac{1.25 \times 10^{4} K}{T}

Energy of activation (in

k c a l

) is:

Q. Rate constant for the decomposition of ethylene oxide into

C H_{4}

and

C O

may be described by the equation,

log [k (s^{- 1})] = 14.34 - \frac{1.25 \times 10^{4}}{T}

.
(a) What is the energy of activation of this reaction?
(b) What is the value of

k

670

K

Q. The rate constant of the first-order reaction may be described by following equation:

log K =

14.34 - \frac{1.25 \times 10^{4}}{T}

, calculate energy of activation.

Q. For a first order reaction

A \to P

, the temperature

(T)

and dependent rate constant

(k)

, was found to follow the equation

log k = - (2000) \frac{1}{T} + 6.0

. What is activation energy?

The first order rate constant for the decomposition of ethyl iodide by the reaction:

$C_{2} H_{5} I (g) \to C_{2} H_{4} (g) + H I (g)$

at $600 K$ is $1.60 \times 10^{- 5} s^{- 1}$ . Its energy of activation is $209 k J m o l^{- 1}$ . The rate constant of the reaction at $700 K$ will be:

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the rate constant for first order decomposition if certain reaction is described by the equation log k = 9.27-7.2×10^-3K/T the activation energy of reaction is ​

the rate constant for first order decomposition if certain reaction is described by the equation log k = 9.27-7.2×10^-3K/T the activation energy of reaction is