Chemistry, asked by tammu3888, 10 months ago

The time required for 10% completion of a first order reaction at 298 K is equal to that required for its 25% completion at 308 K. If the value of A is 4 × 1010 s−1. Calculate k at 318 K and Ea.

Answers

Answered by savageserbs
1

Answer:For a first order reaction,

t = 2.303 / k log a  / a - x

At 298 K,

t = 2.303 / k log 100  / 90

= 0.1054 / k

At 308 K,

t' = 2.303 / k' log 100  / 75

= 2.2877 / k'

According to the question,

t = t'

⇒ 0.1054 / k  =  2.2877 / k'

⇒ k' / k  = 2.7296

From Arrhenius equation,we obtain

To calculate k at 318 K,

It is given that, A = 4 x 1010 s-1, T = 318K

Again, from Arrhenius equation, we obtain

Therefore, k = Antilog (-1.9855)

= 1.034 x 10-2 s -1

Explanation:

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