What is the half life of a first order reaction if time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 h?

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6 h Explanation: k = 2.303/t log((A_0)/(A_t)) Where, A0 is the initial concentration, At is the concentration after time t, t is the time taken. `k = 2.$\frac{303}{12}$ log((0.8)/(0.2)) k = 2.$\frac{303}{12}$ log(4) k = 2.$\frac{303}{12}$ 2log(2) k = 2.$\frac{303}{12}$ xx 0.6020 k = (2.303 xx 0.6020)/12 k = 1.$\frac{384306}{12}$ k ≈ 0.11536 hr−1 t_(1//2) = 0.693/k t_(1//2) = 0.$\frac{693}{0}$.11536 t_(1//2) ≈ 6.01` h The half-life of the first-order reaction is approximately 6 hours.

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