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spin [16.1K]
3 years ago
10

In the first order reaction A → products, the initial concentration of A is 0.1 108M, and 44 s later, 0.0554M. What is the initi

al rate of this reaction? (Initial rate-k[A]). (t %-0.693/k)
Chemistry
1 answer:
lilavasa [31]3 years ago
8 0

Answer : The initial rate of the reaction is, 1.739\times 10^{-3}s^{-1}

Explanation :

First we have to calculate the rate constant of the reaction.

Expression for rate law for first order kinetics is given by :

k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}

where,

k = rate constant  = ?

t = time taken for the process  = 44 s

[A_o] = initial amount or concentration of the reactant  = 0.1108 M

[A] = amount or concentration left time 44 s = 0.0554 M

Now put all the given values in above equation, we get:

k=\frac{2.303}{44}\log\frac{0.1108}{0.0554}

k=0.0157

Now we have to calculate the initial rate of the reaction.

Initial rate = K [A]

At t = 0, [A]=[A_o]

Initial rate = 0.0157 × 0.1108 = 1.739\times 10^{-3}s^{-1}

Therefore, the initial rate of the reaction is, 1.739\times 10^{-3}s^{-1}

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