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Fofino [41]
3 years ago
11

WILL MARK BRAINLIEST AND THANK YOU!! PLEASE HELP!!!

Chemistry
1 answer:
denpristay [2]3 years ago
6 0

Answer:

c

Explanation:

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How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?4247.56.56
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Answer:

6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.

Explanation:

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

Where,

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[A_0] is the initial concentration

Given:

Concentration is decreased to 1.56 % which means that 0.0156 of [A_0] is decomposed. So,

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Thus,

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0.0156=e^{-k\times t}

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k=\frac {ln\ 2}{t_{1/2}}

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t = 6\times t_{1/2}

<u>6 half-lives are required for the concentration of reactant to decrease to 1.56% of its original value.</u>

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