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Arrows disappeared from below added them back to the equations.

??(a) I don't understand ln(No/N)=akt
Is (a) -3.77
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? _____________________

  • Chemistry-DrBob222 -

    I don't know the problem so I don't know what the answer to a is. For the ln(No/N) = akt problem see below.
    You know k = 0.00255/sec
    2IBr ==> I2 + Br2

    ln(No/N) = akt
    No = 1.50M from the problem. That's what you start with.
    N = The M at time t.
    a is the coefficient 2 for IBr.
    k is from above.
    t = 2.5 minutes from the problem but since k is in seconds (I assume the half life given is in seconds) then you must convert 2.5 minutes to seconds. Solve for N to determine the M at time 2.5 minutes.

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