A first order reaction takes `40 mi n ` for `30%` decomposition. Calculate `t_(1//2)`.
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For a first order reaction , `t = (2.303)/(k) "log" ([R]_(0))/([R])` `k = (2.303)/( 40 "min") "log" (100)/(100 -30)` = `(2.303)/(40 "min") "log" (10)/(7)` = `8.918 xx 10^(-3) "min"^(-1)` Therefore , `t_(1//2)` of the decomposition reaction is `t_((1)/(2)) = (0.693)/(k)` = `(0.693)/(8.918 xx 10^(-3)) ` min = `77.7` min (approximately)
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