I have studied your work a bit Mathmike and believe that the source of "error" in your calculations is due to your treatment of the value of "k" as a negative quantity. The "correct" relation for the T (half life) is (ln 2)/(k) = T (the equation H-man provided). Work:
yfinal = 1/2(y-initial)
1. 1/2(y-initial) = y-initial(e^-kt) (note the minus sign attached to k, your equation lacks this key component)
2. Divide out y initial. Moved e^-kt to the denominator on the right side.
3. 1/2 = 1/e^kt
4. Flipped equations.
5. 2 = e^kt
6. ln (2) = kt
7. t half life = ln (2)/k
K by convention is reported as a *positive* quantity (even if the rate is decreasing for the reaction, the value of k is still reported as being positive). To see why, consider that half life reactions are first order reactions and the integrated rate law for that is:
Ln [Xfinal] = - kt + Ln[Xinitial]
Note that if k was negative and you substituted a negative k into this equation, you would have that value times a negative (if k was negative that equals a *positive* slope ultimately which would not do). So k is reported as a positive number (since they decided by convention to indicate the negative slope in the equation rather than have k be a negative number. They probably did this so that people who just see the algebra without substituting any numbers will recognize that the slope for the function is decreasing).
Your thinking is NOT incorrect though I (finally) recognize. If you substitute a negative k into your equation: