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Half-life of first order process

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A reactant undergoes a dissociation reaction A r arrow 2B which follows first order kinetics. The initial concentration of reactant A is .4000 M and after 75.00 hr the concentration of A decreases to 0.0816 M. Determine the half-life of the first order process.

There must be a simple equation for this, but my textbook must assume we would already know it. I can't find it anywhere! Thanks

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This solution is provided in 41 words in an attached .doc file. It provides a simple, brief calculation for finding half-life of a process.

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ln ------------ = -k * t

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