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calculate the half-life of a first- order reaction if the concentration of the reactant is 0.0396 M at 12 seconds after the reaction starts and is 0.00579 M at 47 after the reaction starts. How long does it take for the reactant concentration to decrease to 0.00269 M

  • chemistry -

    ln(No/N) = kt
    No = 0.0396
    N = 0.00579
    k = solve
    t = 47-12 = 35 seconds.
    Solve for k, then
    k = 0.693/t1/2 and solve for t1/2

    ln(No/N) = kt and plug in the new numbers to find time for the 0.00269M to be reached.

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