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After 52.0 min, 36.0% of a compound has decomposed. what is the half life of this reaction assuming first order kinetics?

User Ayu
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1 Answer

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Final answer:

To determine the half-life of a first-order reaction, use the formula t1/2 = (0.693/k) * log(initial concentration / remaining concentration), where k is the rate constant. Substituting the given values, we can solve for t1/2.

Step-by-step explanation:

In a first-order reaction, the concentration of a compound decreases by half in each successive half-life.

Given that 36.0% of the compound has decomposed after 52.0 min, we can use the formula:

t1/2 = (0.693/k)

Where t1/2 is the half-life and k is the rate constant. Since 36.0% of the compound has decomposed, then 1 - 0.36 = 0.64 remains. Hence, the reaction is 64% complete. Substituting the values into the formula:

t1/2 = (0.693/k) * log(initial concentration / remaining concentration)

t1/2 = (0.693/k) * log(1 / 0.64)

By solving for t1/2, we can determine the half-life of the reaction assuming first-order kinetics.

t1/2 = ????

User Iajrz
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