ChemistryDrBob222
posted by David .
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 halflife 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 ratedetermining step? ______________
What is the molecularity of the ratedetermining step? _____________________

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.
Respond to this Question
Similar Questions

Chemistry
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? 
Chemistry
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? 
Chemistry
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? 
ChemistryDrBob222
Arrows disappeared from below added them back to the equations. 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? 
ChemistryDrBob222
Arrows disappeared from below added them back to the equations. ? 
AP CHEMISTRY
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.590 mol IBr in a 2.50L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2? 
chem
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.570 mol IBr in a 2.50L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2? 
Chemistry
A sealed 1.0L flask is charged with .500mol I2 and .500mol Br2 and an equilibrium reaction esues: I2(g)+Br2(g)=2IBr(g) When the container contents achieve equilibrium, the flask contains .84 mol of IBr. What is the value of the eqilibrium … 
chemistry
At a certain temperature, Keq is 4.13 x 10^5 for the equilibrium: 2IBr(g) ↔ I2(g) + Br2(g) Assume that the equilibrium is established at the above temperature by adding only the reactant to the reaction flask. What are the concentrations … 
chemistry
Will you help me use the half reaction method to balance these equations. I need to add water molecules and hydrogen ions in acid solutions. I also need to keep the balanced equations in net ionic form. thanks 1) Cl(aq) + NO3(aq) …