A particular reactant decomposes with a half-life of 153 seconds when its initial concentration is 0.298 M. The same reactant decomposes with a half-life of 237 seconds when its initial concentration is 0.192 M. Determine the reaction order. - \( \circ \) 0 - \( \circ \) 2 - \( \circ \) 1 What is the value and units of the rate constant for this reaction? \( k = \) [_____________] Units [_____________]

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A particular reactant decomposes with a half-life of 153 seconds when its initial concentration is 0.298 M. The same reactant decomposes with a half-life of 237 seconds when its initial concentration is 0.192 M.

Determine the reaction order.

- \( \circ \) 0 
- \( \circ \) 2 
- \( \circ \) 1 

What is the value and units of the rate constant for this reaction?

\( k = \) [_____________] Units [_____________]
Transcribed Image Text:A particular reactant decomposes with a half-life of 153 seconds when its initial concentration is 0.298 M. The same reactant decomposes with a half-life of 237 seconds when its initial concentration is 0.192 M. Determine the reaction order. - \( \circ \) 0 - \( \circ \) 2 - \( \circ \) 1 What is the value and units of the rate constant for this reaction? \( k = \) [_____________] Units [_____________]
Expert Solution
Step 1

The half-life of the second-order reaction:
For the second-order reaction, the half-life time is inversely proportional to the initial concentration of the reactant. The half-life time is given by:

t12 = 1k2 Aot12 α 1[Ao]

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