posted by David on .
The decomposition of IBr(g)into I2 (g) and Br2 (g) is first order in IBr with k = 0.00255/sec.
(a)Starting with [IBr] = 1.50M, what will [IBr] become after 2.50 minutes?
(b)How long, in minutes, will it take for [IBr] to go from 0.500M to 0.100M?
(c)What is the half-life for this reaction in seconds?
(d)Enough IBr is added to an evacuated container to make [IBr] = 0.350M. How long will it take [I2] = 0.100M?
(e) The following mechanism has been proposed for the reaction above:
(step 1)IBr (g) ¨ I (g) + Br (g)(step 2)IBr(g) + Br (g) ¨ Br2(g) +I (g)(step 3)I (g) + I (g) ¨ I2 (g)
Based on the rate law described above, which step is the rate-determining step? ______________
What is the molecularity of the rate-determining step? _____________________