For the first-order reaction
log([A]0/[A]) = kt/2.303 and t1/2 = 0.693/k
Find k
log (10.9/7.4*10-3) = k*9.6/2.303
k = 0.76 s-1
Find t1/2
t1/2 = 0.693/0.76 = 0.912 s
Answer: 0.912 s
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